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Ch6.1 The Nature of Energy Energy – the capacity to do work or to produce heat. Law of Conservation of Energy – energy can be converted from one form to.

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Presentation on theme: "Ch6.1 The Nature of Energy Energy – the capacity to do work or to produce heat. Law of Conservation of Energy – energy can be converted from one form to."— Presentation transcript:

1 Ch6.1 The Nature of Energy Energy – the capacity to do work or to produce heat. Law of Conservation of Energy – energy can be converted from one form to another, but can be neither created or destroyed. 1st Law of thermodynamics – the energy of the universe is constant. Potential energy – stored energy due to position or composition Kinetic energy – energy of motion KE = ½mv2 Heat – (a form of energy) transfer of energy due to a temp difference Temperature – property that reflects the randomness of the particles (NOT a form of energy)

2 Chemical energy Exothermic reaction – CH4(g) + O2(g) 

3 Chemical energy Exothermic reaction – heat flows out of the system (feel hot) CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) + energy

4 Chemical energy Exothermic reaction – heat flows out of the system (feel hot) CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) + energy In any exothermic reaction, some of the potential energy stored in chemical bonds is converted to thermal energy.

5 Endothermic reaction –
N2(g) + O2(g) 

6 Endothermic reaction – absorb heat from their surroundings (feel cold)
- heat flows into the system N2(g) + O2(g) + energy  2NO(g)

7 1st Law of Thermodynamics – the energy of the universe is constant.
ΔE = q + w Internal heat work energy energy “All energy movements reflect the system’s point of view.” ΔE = Internal energy of the system increased ΔE = – Internal energy of the system decreased q = + Heat flowed into the system q = – Heat flowed out of the system w = + The surroundings do work on the system w = – The system does work on the surroundings

8 Ex1) Calculate ΔE for a system undergoing an endothermic process
in which 15.6kJ of heat flows and where 1.4kJ of work is done on the system.

9 Work associated with gases:
Pressure: Work:

10 Ex2) Calc the work associated with the expansion of a gas
from 46L to 64L at a constant pressure of 15 atm.

11 1.3x108J of heat are added. Atmospheric pressure is 1.0 atm.
Ex3) A balloon is being inflated to its full extent by heating the air inside it. The volume changes from 4.00x106L to 4.50x106L when 1.3x108J of heat are added. Atmospheric pressure is 1.0 atm. Calculate ΔE for the process. Ch6 HW#1 p283 21,23,25,26

12 Ch6 HW#1 p283 21,23,25,27 21. Calculate ΔE for each of the following cases. a. q = +51 kJ, w = -15kJ b. q = +100 kJ, w = -65kJ c. q = -65kJ, w = -20kJ d. In which of these does the system do work on the surroundings?

13 Ch6 HW#1 p283 21,23,25,26 21. Calculate ΔE for each of the following cases. a. q = +51 kJ, w = -15kJ b. q = +100 kJ, w = -65kJ c. q = -65kJ, w = -20kJ d. In which of these does the system do work on the surroundings? ΔE = q + w a. ΔE = +51 kJ + (-15kJ) = +36kJ (Internal energy increases) b. ΔE = +100 kJ + (-65kJ) = +35kJ (Internal energy increases) c. ΔE = -65kJ + (-20kJ) = -85kJ (Internal energy decreases) d. All 3 have w = (-) so all systems did work on the surroundings

14 23. A gas absorbs 45kJ of heat and does 29kJ of work. Calculate ΔE.
ΔE = q + w

15 23. A gas absorbs 45kJ of heat and does 29kJ of work. Calculate ΔE.
ΔE = q + w = (+45kJ) + (-29kJ) = +16kJ (increase)

16 25. The volume of an ideal gas is decreased from 5.0 L to 5.0 mL
at a constant pressure of 2.0 atm. Calculate the work associated with this process. ΔV = (0.005L – 5L) = L

17 25. The volume of an ideal gas is decreased from 5.0 L to 5.0 mL
at a constant pressure of 2.0 atm. Calculate the work associated with this process. ΔV = (0.005L – 5L) = L W = –P. ΔV = –(202.6kPa). (-4.995L) = J = kJ (work done on the gas!)

18 26. Consider the mixture of air and gasoline vapor in a cylinder with
a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is conserved into work to push back the piston. ΔV = (V2 – 0.040L) q  W =

19 26. Consider the mixture of air and gasoline vapor in a cylinder with
a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is conserved into work to push back the piston. ΔV = (V2 – 0.040L) q  W = –950J (expands – gas doing work) W = –P. ΔV –950J = –(86.6kPa). ΔV ΔV = 10.97L 10.97L = (V2 – 0.040L) V2 = 11.0L

20 Ch6.1B – PV Diagrams ‘A closed system at equilibrium has no tendency to undergo spontaneous macroscopic change.” 4 basic models where a closed system is changed: Constant Can change Equations Implications Thermo Eqn 1. Isothermal 2. Isobaric 3. Isovolumetric 4. Adiabatic (no heat transferred to or from a system.) Work equation: (Units: ______, or ______, or ______)

21 Ch6.1B – PV Diagrams ‘A closed system at equilibrium has no tendency to undergo spontaneous macroscopic change.” 4 basic models where a closed system is changed: Constant Can change Equations Implications Thermo Eqn 1. Isothermal T V, P V1P1 = V2P2 If ∆T = 0, q = W then ∆E=0 2. Isobaric P V, T ∆E = q + W 3. Isovolumetric V P, T No work ∆E = q done. 4. Adiabatic nothing V, P, T Q = 0 ∆E = W (no heat transferred to or from a system.) Work equation: W = –P . ∆V (Units: Joules, or Pa.m3, or kPa.L)

22 50 Work = (area under the PV curve.)
Decide +/- based on direction P 30 (Pa) 20 10 V (m3) 101.3 P (kPa) V (L) 150 P 100 (Mpa) 50 V(cm3)

23 50 Work = –(area under the PV curve.)
Decide +/- based on direction P W = ½(3m3)(40N/m2) (Pa) = –60J 10 V (m3) W = (101.3kPa)(3L) P (1kPa  1000Pa) (kPa) = –303.9J (1L  0.001m3) V (L) 150 No work done P (Isovolumetric) (Mpa) (1 Mpa 1,000,000Pa) (1cm3  m3) V(cm3)

24 Ex3) A cylinder contains 264
Ex3) A cylinder contains moles of a monatomic gas that is initially at state A at standard temperature, and a pressure of 6x105Pa. a. What volume does the gas occupy? 6 b. Please graph state A c. A certain amount of heat is added, P 4 bringing the gas isobarically to state B, (x105 Pa) 3 at a volume of 3m3, while its internal energy 2 is increased by 400kJ. How much heat was added? 1 Please graph state B V(m3) d. The gas is brought isothermally to state C, where the pressure was reduced to 3x105Pa. What is the new volume? Please graph state C. Ch6 HW#2 1 – 4

25 Ex3) A cylinder contains 264
Ex3) A cylinder contains moles of a monatomic gas that is initially at state A at standard temperature, and a pressure of 6x105Pa. a. What volume does the gas occupy? 6 b. Please graph state A c. A certain amount of heat is added, P 4 bringing the gas isobarically to state B, (x105 Pa) 3 at a volume of 3m3, while its internal energy 2 is increased by 400kJ. How much heat was added? 1 Please graph state B V(m3) d. The gas is brought isothermally to state C, where the pressure was reduced to 3x105Pa. What is the new volume? Please graph state C. a. PV=nRT c. ∆E = q + W W = –(area) = (+2m3)(6x105Pa) = –1,200,000J (+400,000J) = q + (–1,200,000J) + q = +1,600,000J d. VB = 3m VC = ? VB. PB = VC. PC PB = 6x105Pa PC = 3x105Pa (3)(6) = (VC)(3) TB = ? same TC = ? VC =6m3

26 Ch6 HW#2 1 – 4 1. A quantity of gas in a cylinder sealed with a piston absorbs 4186J of heat as it expands by 15L at constant pressure. If the internal energy increases by 286J, what was the constant pressure? 2. A cylinder sealed with a piston contains 20.0m3 of pure oxygen at standard pressure. The gas is then forced into a tiny high pressure container of negligible volume. What is the amt of work done on the gas? What do you think happens to the temp of the gas as it is compressed?

27 Ch6 HW#2 1 – 4 1. A quantity of gas in a cylinder sealed with a piston absorbs 4186J of heat as it expands by 15L at constant pressure. If the internal energy increases by 286J, what was the constant pressure? q = J ∆E = q + w ∆V = + 15L  0.015m3 w = (+286J) – (+4186J) ∆U = +286J w = – 3890J 2. A cylinder sealed with a piston contains 20.0m3 of pure oxygen at standard pressure. The gas is then forced into a tiny high pressure container of negligible volume. What is the amt of work done on the gas? What do you think happens to the temp of the gas as it is compressed?

28 Compression of a gas increases temp.
Ch6 HW#2 1 – 4 1. A quantity of gas in a cylinder sealed with a piston absorbs 4186J of heat as it expands by 15L at constant pressure. If the internal energy increases by 286J, what was the constant pressure? q = J ∆E = q + w ∆V = + 15L  0.015m3 w = (+286J) – (+4186J) ∆U = +286J w = – 3890J 2. A cylinder sealed with a piston contains 20.0m3 of pure oxygen at standard pressure. The gas is then forced into a tiny high pressure container of negligible volume. What is the amt of work done on the gas? What do you think happens to the temp of the gas as it is compressed? ∆V = –20.0m W = – P. ∆V P = 101,300Pa = –(101,300Pa)(– 20m3) W = ? = +2,026,000J (work done on the gas) Compression of a gas increases temp.

29 3. A gas experiences a change from state I to state F
3. A gas experiences a change from state I to state F. Determine the work done. 4. A piston with a cross-sectional area of 0.50m2 seals a gas within a cylinder at a pressure of 0.30MPa. 10kJ of heat is gradually added to the cylinder, and the piston rises 6.5cm as the gas expands isobarically. What is the work done by the gas? What is the change in internal energy? A = 0.50m2 h = 6.5cm 6 F P (Mpa) 3 I 1 V (cm3)

30 3. A gas experiences a change from state I to state F
3. A gas experiences a change from state I to state F. Determine the work done. 6 F Work = P = 12J (Mpa) 3 2 I 1 V (cm3) 4. A piston with a cross-sectional area of 0.50m2 seals a gas within a cylinder at a pressure of 0.30MPa. 10kJ of heat is gradually added to the cylinder, and the piston rises 6.5cm as the gas expands isobarically. What is the work done by the gas? What is the change in internal energy? 3 1 2 A = 0.50m2 h = 6.5cm

31 3. A gas experiences a change from state I to state F
3. A gas experiences a change from state I to state F. Determine the work done. 6 F Work = P = 12J (Mpa) 3 2 I 1 V (cm3) 4. A piston with a cross-sectional area of 0.50m2 seals a gas within a cylinder at a pressure of 0.30MPa. 10kJ of heat is gradually added to the cylinder, and the piston rises 6.5cm as the gas expands isobarically. What is the work done by the gas? What is the change in internal energy? A = 0.50m2 ∆V=A. ∆h=(.50m2)(.065m) = m3 h = 6.5cm W = – P. ∆V = (0.3x106Pa)( m3) = – 9750J ∆E = q + W = (+10,000) + (– 9750) = +250J 3 1 2

32 Ch6.1C – PV Diagrams Ex1) The graph shows P vs V for 2 moles of gas cycling from state A to B. The internal energy increases by 400J. a. Calc work done b. Is heat added or removed? How much? P c. The pressure is reduced to 200Pa (Pa) A B isovolumetrically as gas goes from state B to state C. Please graph state C d. The graph is compressed isothermally to state A Draw the lines to represent the cycle. V (m3) e. Is heat added or removed from C  A? How much?

33 Ex1) The graph shows P vs V for 2 moles of gas cycling from state A to B.
The internal energy increases by 400J. a. Calc work done b. Is heat added or removed? How much? P c. The pressure is reduced to 200Pa (Pa) A B isovolumetrically as gas goes from state B to state C. Please graph state C C d. The graph is compressed isothermally to state A Draw the lines to represent the cycle. V (m3) e. Is heat added or removed from C  A? How much? a. W = P. ∆V = (600Pa)(+6m3) = +3600J b. Added: Why else would the gas expand? Q = W + ∆U = +3600J + (+400J) = +4000J c. isovolumetric d. isothermal – P and V can change, while ∆T = 0, so ∆U = 0. e. Heat is removed. Q = W + ∆U = W + 0 Q = WorkCA = (Area) = -2400J (Work is (-) becuz the gas is compressed by outside force. Work done on the gas.)

34 Ex2) A piston with a radius of 0
Ex2) A piston with a radius of 0.05m seals a cylinder that contains a gas at a pressure of 101.3kPa. 100J of heat is added to the cylinder, and the piston rises 0.04m isobarically. a. How much work is done by the gas? h b. What is its change in internal energy? The total pressure exerted on the gas increases to 107.7kPa. c. If the piston seals 1m3, when the pressure increased, and the piston lowers isothermally, what is the new volume? Ch6 HW#3 5 – 8

35 Ex2) A piston with a radius of 0
Ex2) A piston with a radius of 0.05m seals a cylinder that contains a gas at a pressure of 101.3kPa. 100J of heat is added to the cylinder, and the piston rises 0.04m isobarically. a. How much work is done by the gas? h b. What is its change in internal energy? The total pressure exerted on the gas increases to 107.7kPa. c. If the piston seals 1m3, when the pressure increased, and the piston lowers isothermally, what is the new volume? a. ∆V = A. ∆h = π(.05m)2(+.04m) = m3 W = – P. ∆V = – (101,300Pa)( m3) = – 31.8J b. ∆U = q + W = (+100J) + (– 31.8J) = 68J c. V1 = 1 m V2 = ___m V1. P1 = V2. P2 P1 = 101,300Pa P2 = 107,700Pa (1m3)(101,300Pa) = V2(107,700Pa) T1 = ? same T2 = ? V2 = .9m3

36 Ch6 HW#3 5 – 8 1. Given that we have 1200 cm3 of helium at 15°C and 99 kPa, what will be its volume at STP? 2. Three moles of a gas are injected into an evacuated container, with a fixed volume, and maintained at a temp of 60°C. If the pressure increases to 103,200 kPa what volume is the container? PV = nRT

37 Ch6 HW#3 5 – 8 1. Given that we have 1200 cm3 of helium at 15°C and 99 kPa, what will be its volume at STP? 2. Three moles of a gas are injected into an evacuated container, with a fixed volume, and maintained at a temp of 60°C. If the pressure increases to 103,200 kPa what volume is the container? PV = nRT

38 Ch6 HW#3 5 – 8 1. Given that we have 1200 cm3 of helium at 15°C and 99 kPa, what will be its volume at STP? 2. Three moles of a gas are injected into an evacuated container, with a fixed volume, and maintained at a temp of 60°C. If the pressure increases to 103,200 kPa what volume is the container? PV = nRT

39 3. A 0.05 m3 volume of gas absorbs 10 kJ of heat and expands to a volume
of 0.15 m3, while remaining at a constant pressure. During the process, the internal energy increases by 4500 J. What was the pressure? ∆V = +.10m3 q = +10kJ ∆E = +4.5kJ P = ?

40 3. A 0.05 m3 volume of gas absorbs 10 kJ of heat and expands to a volume
of 0.15 m3, while remaining at a constant pressure. During the process, the internal energy increases by 4500 J. What was the pressure? ∆V = .10m3 W = ∆U – q = (+4.5kJ) – (+10kJ) = – 5.5kJ = – 5500J Q = +10kJ ∆U = +4.5kJ P = ? 4. A piston with a cross-sectional area of 0.10 m2 seals a cylinder that contains a gas at a pressure of 100 kPa J of heat are removed from the cylinder, and the piston falls 0.05 m isobarically. a. How much work is done on the gas? b. What is the change in internal energy? c. If the gas is then heated, so that its absolute temperature doubles, what is the new volume of the cylinder?

41 4. A piston with a cross-sectional area of 0
4. A piston with a cross-sectional area of 0.10 m2 seals a cylinder that contains a gas at a pressure of 100 kPa J of heat are removed from the cylinder, and the piston falls 0.05 m isobarically. a. How much work is done on the gas? ∆V=A. ∆h = (.1m2)(–.05m)= –0.005m3 W = – P. ∆V = b. What is the change in internal energy? ∆E = q + W = c. If the gas is then heated, so that its absolute temperature doubles, what is the new volume of the cylinder?

42 4. A piston with a cross-sectional area of 0
4. A piston with a cross-sectional area of 0.10 m2 seals a cylinder that contains a gas at a pressure of 100 kPa J of heat are removed from the cylinder, and the piston falls 0.05 m isobarically. a. How much work is done on the gas? ∆V=A. ∆h = (.1m2)(–.05m)= –0.005m3 W = – P. ∆V = –(100,000Pa)(– 0.005m3) = +500J b. What is the change in internal energy? ∆E = q + W = c. If the gas is then heated, so that its absolute temperature doubles, what is the new volume of the cylinder?

43 4. A piston with a cross-sectional area of 0
4. A piston with a cross-sectional area of 0.10 m2 seals a cylinder that contains a gas at a pressure of 100 kPa J of heat are removed from the cylinder, and the piston falls 0.05 m isobarically. a. How much work is done on the gas? ∆V=A. ∆h = (.1m2)(–.05m)= –0.005m3 W = – P. ∆V = –(100,000Pa)(– 0.005m3) = +500J b. What is the change in internal energy? ∆E = q + W = (-200J) + (+500J) = +300J c. If the gas is then heated, so that its absolute temperature doubles, what is the new volume of the cylinder?

44 4. A piston with a cross-sectional area of 0
4. A piston with a cross-sectional area of 0.10 m2 seals a cylinder that contains a gas at a pressure of 100 kPa J of heat are removed from the cylinder, and the piston falls 0.05 m isobarically. a. How much work is done on the gas? ∆V=A. ∆h = (.1m2)(–.05m)= –0.005m3 W = – P. ∆V = –(100,000Pa)(– 0.005m3) = +500J b. What is the change in internal energy? ∆E = q + W = (-200J) + (+500J) = +300J c. If the gas is then heated, so that its absolute temperature doubles, what is the new volume of the cylinder?

45 Ch6.2A – Enthalpy Enthalpy, H – the ‘heat content’ of a substance
defined as: H = E + PV H is related to q. Officially: at constant pressure q = H For practical purposes: q is the heat measured in an experiment H is the heat related to a chem rxn.

46 Enthalpy, H – the ‘heat content’ of a substance
ΔH = Hproducts – Hreactants Exothermic reaction: Enthalpy time

47 Enthalpy, H – the ‘heat content’ of a substance
ΔH = Hproducts – Hreactants Endothermic reaction: Enthalpy time

48 Ex1) When 1 mol of methane is burned at constant pressure,
890kJ of energy is released as heat. Calculate ΔH for a process in which a 5.8g sample is burned.

49 Ex2) a. Write an eqn for the combustion of ethanol, C2H5OH.
1235 kJ of heat is given off. b. Draw an energy diagram. c. How much heat is produced when 12.5g of ethanol reacts? Ch6 HW#4 p283 29,30,31,33,34

50 Ch6 HW#4 p283 29,30,31,33,34 29. The equation for the fermentation of glucose to alcohol and carbon dioxide is C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is -67kJ. Is the reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?

51 Ch6 HW#4 p283 29,30,31,33,34 29. The equation for the fermentation of glucose to alcohol and carbon dioxide is C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(g) + 67kJ exothermic heat is evolved as the reaction occurs?

52 30. The reaction SO3(g) + H2O(l) → H2SO4(aq)
is the last step in the commercial production of sulfuric acid. The enthalpy change for this reaction is -227 kJ. In the designing a sulfuric acid plant, is it necessary to provide for heating or cooling of the reaction mixture? Explain.

53 30. The reaction SO3(g) + H2O(l) → H2SO4(aq)
is the last step in the commercial production of sulfuric acid. The enthalpy change for this reaction is -227 kJ. In the designing a sulfuric acid plant, is it necessary to provide for heating or cooling of the reaction mixture? Explain. SO3(g) + H2O(l) → H2SO4(aq) kJ Cool the plant!

54 31. Are the following processes exothermic or endothermic?
a. When solid KBr is dissolved in water, the solution gets colder. KBr(s) + _____ → K+(aq) + Br-(aq) + _____ b. Natural gas (CH4) is burned in a furnace. CH4(g) + O2(g) + _____ → CO2(g) + H2O(g) + _____ c. When concentrated H2SO4 is added to water, the solution gets very hot. H2SO4(aq) + _____ → 2H+(aq) + SO42-(aq) + _____ d. Water is boiled in a teakettle. H2O(l) + _____ → H2O(g) + _____

55 31. Are the following processes exothermic or endothermic?
a. When solid KBr is dissolved in water, the solution gets colder. KBr(s) + heat → K+(aq) + Br-(aq) b. Natural gas (CH4) is burned in a furnace. CH4(g) + O2(g) → CO2(g) + H2O(g) + heat c. When concentrated H2SO4 is added to water, the solution gets very hot. H2SO4(aq) + _____ → 2H+(aq) + SO42-(aq) + _____ d. Water is boiled in a teakettle. H2O(l) + _____ → H2O(g) + _____

56 31. Are the following processes exothermic or endothermic?
a. When solid KBr is dissolved in water, the solution gets colder. KBr(s) + heat → K+(aq) + Br-(aq) b. Natural gas (CH4) is burned in a furnace. CH4(g) + O2(g) → CO2(g) + H2O(g) + heat c. When concentrated H2SO4 is added to water, the solution gets very hot. H2SO4(aq) → 2H+(aq) + SO42-(aq) + heat d. Water is boiled in a teakettle. H2O(l) + heat → H2O(g)

57 33. For the reaction S(s) + O2(g) → SO2(g) ΔH = -296 kJ/mol a. How much heat is evolved when 275g sulfur is burned in excess O2? b. How much heat is evolved when 25mol sulfur is burned in excess O2? c. How much heat is evolved when 150. g sulfur dioxide is produced?

58 33. For the reaction S(s) + O2(g) → SO2(g) ΔH = -296 kJ/mol a. How much heat is evolved when 275g sulfur is burned in excess O2? q = b. How much heat is evolved when 25mol sulfur is burned in excess O2? c. How much heat is evolved when 150. g sulfur dioxide is produced?

59 33. For the reaction S(s) + O2(g) → SO2(g) ΔH = -296 kJ/mol a. How much heat is evolved when 275g sulfur is burned in excess O2? q = b. How much heat is evolved when 25mol sulfur is burned in excess O2? c. How much heat is evolved when 150. g sulfur dioxide is produced?

60 33. For the reaction S(s) + O2(g) → SO2(g) ΔH = -296 kJ/mol a. How much heat is evolved when 275g sulfur is burned in excess O2? q = b. How much heat is evolved when 25mol sulfur is burned in excess O2? c. How much heat is evolved when 150. g sulfur dioxide is produced?

61 34. The overall reaction in commercial heat packs can be represented
as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = -1652kJ a. About how much heat is released when 4.00 mol iron is reacted with excess O2? b. How much heat is released when 1.00 mol Fe2O3 is produced? c. How much heat is released when 1.00 g iron is reacted with excess O2? d. How much heat is released when 10.0 g Fe and 2.00 g O2 are reacted?

62 34. The overall reaction in commercial heat packs can be represented
as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = -1652kJ a. About how much heat is released when 4.00 mol iron is reacted with excess O2? b. How much heat is released when 1.00 mol Fe2O3 is produced? c. How much heat is released when 1.00 g iron is reacted with excess O2? d. How much heat is released when 10.0 g Fe and 2.00 g O2 are reacted?

63 34. The overall reaction in commercial heat packs can be represented
as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = -1652kJ c. How much heat is released when 1.00 g iron is reacted with excess O2? d. How much heat is released when 10.0 g Fe and 2.00 g O2 are reacted? (excess Fe) released

64 Ch6.2B – Calorimetry Calorimetry – the measure of heat flow
Heat Capacity (C) – of heat flow to a substance, compared to its temp change. (In lab 6.2 you will find C for a foam cup)

65 Calorimetry – the measure of heat flow
Heat Capacity (C) – of heat flow to a substance, compared to its temp change. Molar Heat Capacity – heat flow per mole, per temp change units:

66 Calorimetry – the measure of heat flow
Heat Capacity (C) – of heat flow to a substance, compared to its temp change. Specific heat capacity (s or Cp) – measure of heat flow to 1 gram of a substance, compared to its temp change. Exs: (In lab 6.1 you will find the Cp for an unknown…per gram of it)

67 Ex1) A 46.2 g sample of copper is heated to 95.4˚C and then placed in
a calorimeter containing 75.0 g water at 19.6˚C. The final temperature of the metal and water is 21.8˚C. Calculate the specific heat capacity of copper, assuming that all the heat lost by the copper is gained by water.

68 Ex2) 50ml of 1.00M HCl at 25.0oC is mixed with 50ml of 1.00M NaOH
at 25.0oC in a calorimeter. The temp of the mix reaches 31.9oC. If the Cp of the solution is , and the density of the final soln is 1.0 g/ml, calc the enthalpy change per mole for this neutralization reaction. Ch6 HW#5 p284 27,42,43

69 Ex2) 50ml of 1.00M HCl at 25.0oC is mixed with 50ml of 1.00M NaOH
at 25.0oC in a calorimeter. The temp of the mix reaches 31.9oC. If the Cp of the solution is , and the density of the final soln is 1.0 g/ml, calc the enthalpy change per mole for this neutralization reaction. HCl + NaOH  NaCl + HOH + ______J 0.05mol mol (100ml)(1.0g/ml) = 100g q = (100g)(4.18 J/g.0C)(5.90C) = 2466J ΔH = 2466J/0.10mol = 24,660J Ch6 HW#5 p284 27,42,43

70 q = ΔH = W = –P.ΔV = ΔE = q + W = Ch6 HW#5 p284 27,42,43
27. A balloon filled with 39.1 mol helium has a volume of 876L a 0.0˚C and 1.00 atm pressure. The temperature of the balloon is increased to 38.0˚C as it expands to a volume of 998 L, the remaining pressure remaining constant. Calculate q, w, ΔE for the helium in the balloon. (The molar heat capacity for helium gas is 20.8 J/˚C·mol.) n = 39.1 mol C/mol = 20.8 J/˚C·mol Vi = 876L Vf = 998 L Ti = 0.0˚C Tf = 38.0˚C P = 1.00 atm = 101.3kPa (stays const) q = ΔH = W = –P.ΔV = ΔE = q + W =

71 q = ΔH = W = –P.ΔV = –(101.3kPa)(122L) = –12,359J
27. A balloon filled with 39.1 mol helium has a volume of 876L a 0.0˚C and 1.00 atm pressure. The temperature of the balloon is increased to 38.0˚C as it expands to a volume of 998 L, the remaining pressure remaining constant. Calculate q, w, ΔE for the helium in the balloon. (The molar heat capacity for helium gas is 20.8 J/˚C·mol.) n = 39.1 mol C/mol = 20.8 J/˚C·mol Vi = 876L Vf = 998 L Ti = 0.0˚C Tf = 38.0˚C P = 1.00 atm = 101.3kPa (stays const) q = ΔH = W = –P.ΔV = –(101.3kPa)(122L) = –12,359J ΔE = q + W = 30,905J + (-12,359J) = +18,546J

72 42. A 15.0 g sample of nickel metal is heated to 100˚C and dropped
into 55.0 g of water, initially at 23˚C. Assuming that all the heat lost by the nickel is absorbed by the water, calculate the final temp of the nickel and water. (Specific heat of nickel = J/˚C · g) Heat lost by nickel = Heat gained by water – m.cpNi.ΔT = + m.cpw.ΔT

73 42. A 15.0 g sample of nickel metal is heated to 100˚C and dropped
into 55.0 g of water, initially at 23˚C. Assuming that all the heat lost by the nickel is absorbed by the water, calculate the final temp of the nickel and water. (Specific heat of nickel = J/˚C · g) Heat lost by nickel = Heat gained by water – m.cpNi.ΔT = + m.cpw.ΔT

74 43. A 150. 0-g sample of metal at 75. 0˚C is added to 150
43. A g sample of metal at 75.0˚C is added to g of H2O at 15.0˚C. The temperature of water rises to 18.3˚C. Calculate the specific heat capacity of the metal, assuming that all the heat lost is gained by the water. Heat lost by nickel = Heat gained by water – m.cpNi.ΔT = + m.cpw.ΔT

75 43. A 150. 0-g sample of metal at 75. 0˚C is added to 150
43. A g sample of metal at 75.0˚C is added to g of H2O at 15.0˚C. The temperature of water rises to 18.3˚C. Calculate the specific heat capacity of the metal, assuming that all the heat lost is gained by the water. Heat lost by nickel = Heat gained by water – m.cpNi.ΔT = + m.cpw.ΔT

76 Ch6.2C More Calorimetry and Enthalpy
Ex1) 1.00L of 0.10M Ba(NO3)2 solution at 25.0oC is mixed with 1.00L of 0.10M Na2SO4 soln at 25.0oC in a calorimeter. A ppt forms. The temp of the mix reaches 28.1oC. If the Cp of the solution is , and the density of the final soln is 1.0 g/ml, calc the enthalpy change per mole of ppt.

77 Ex2) 15.00 g of CaCl2 at 21.1oC is dissolved in 50.0mL of water
also at 21.1oC in a calorimeter. The temp of the mix reaches 42.5oC. Heat absorbed by the calorimeter is negligible. If the Cp of the solution is , and the density of the final soln is 1.0 g/ml, calc the enthalpy change per mole of ppt. Ch6 HW#6 p284 37,45,47,48

78 Lab6.1 Calorimetry - unknown end of period. - lab write up due 2 days - Ch6 HW#6 due tomorrow

79 Ch6 HW#6 p284 37,45,47,48 37. The specific heat capacity of aluminum is 0.9 J/˚C·g. a. Calculate the energy needed to raise the temperature of an 8.5x102 g block of aluminum from 22.8˚C to 94.6˚C. cp = 0.9 J/˚C·g m = 8.5x102 g ΔT = 71.8˚C energy needed = ? q = m.cp.ΔT b. Calculate the molar heat capacity of aluminum.

80 37. The specific heat capacity of aluminum is 0.9 J/˚C·g.
a. Calculate the energy needed to raise the temperature of an 8.5x102 g block of aluminum from 22.8˚C to 94.6˚C. cp = 0.9 J/˚C·g m = 8.5x102 g ΔT = 71.8˚C energy needed = ? b. Calculate the molar heat capacity of aluminum.

81 37. The specific heat capacity of aluminum is 0.9 J/˚C·g.
a. Calculate the energy needed to raise the temperature of an 8.5x102 g block of aluminum from 22.8˚C to 94.6˚C. cp = 0.9 J/˚C·g m = 8.5x102 g ΔT = 71.8˚C energy needed = ? b. Calculate the molar heat capacity of aluminum.

82 NIE: Ag+(aq) + Cl-(aq) →AgCl (s)
45. In a coffee-cup calorimeter, 50.0 mL of M AgNO3 and 50.0 mL of M HCl are mixed to yield the following reaction: NIE: Ag+(aq) + Cl-(aq) →AgCl (s) The two solutions were initially at 22.60˚C, and the final temperature is 23.40˚C. Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 g and has a specific heat capacity of 4.18 J/˚C·g. ΔT = 0.8 ˚C Ag+(aq) + Cl-(aq) water AgCl (s) + heat (ΔH) cp = 4.18 J/˚C·g V=0.05L V=0.05L m = 100g ΔH: kJ/mol = ? (q/n) M=0.100M M=0.100M

83 cp = 4.18 J/˚C·g n = 0.005mol of each → n = 0.005mol product
ΔT = 0.8 ˚C Ag+(aq) + Cl-(aq) water AgCl (s) + ____J cp = 4.18 J/˚C·g n = 0.005mol of each → n = 0.005mol product ΔH: kJ/mol = ? (q/n) g total soln q = + m.cp.ΔT 0.005 moles yielded 334J of energy to the 100g of solution, so how much heat would 1mol yield?

84 cp = 4.18 J/˚C·g n = 0.005mol of each → n = 0.005mol product
ΔT = 0.8 ˚C Ag+(aq) + Cl-(aq) water AgCl (s) + heat (q) cp = 4.18 J/˚C·g n = 0.005mol of each → n = 0.005mol product kJ/mol = ? (q/n) g total soln q = + m.cp.ΔT While the entire mass of solution had its temperature changed because of the rxn, only the moles of the rxn provided the heat! moles yielded 334J of energy to the 100g of solution, - 1 mol of reactants woulda provided 66,900J to the solution!

85 m=11g m=125g 47.Consider the dissolution of CaCl2:
CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔH = kJ An 11.0g sample of CaCl2 is dissolved in 125 g of water, with both substances at 25.0˚C. Calculate the final temperature of the solution assuming no heat lost to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/˚C·g CaCl2(s) water Ca2+(aq) + 2Cl-(aq) kJ m=11g m=125g Ti = 25C Ti = 25C per 1 mol CaCl2

86 m=11g m=125g 47. CaCl2(s) water Ca2+(aq) + 2Cl-(aq) + 81.5 kJ
Ti = 25C Ti = 25C per 1 mol CaCl2 q = – m.cp.ΔT

87 2HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2H2O(l) ΔH = -118 kJ
48. Consider the reaction 2HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2H2O(l) ΔH = -118 kJ Calculate the heat when mL of M HCl is mixed with 300.0 mL of M Ba(OH)2. Assuming that the temperature of both solutions was initially 25.0˚C and that the final mixture has a mass of g and a specific heat capacity of 4.18 J/˚C · g, calculate the final temperature of the mixture. 2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l) +118 kJ 0.10mol mol Ti = 25.0˚C this will run out q = – m.cp.ΔT

88 0.10mol 0.15mol total mass = 400g Ti = 25.0˚C q = – m.cp.ΔT
HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l) +118 kJ 0.10mol mol total mass = 400g Ti = 25.0˚C q = – m.cp.ΔT Tf = 32.1˚C

89 Ch6.3 – Hess’s Law In going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or a series of steps. 1 step: N2(g) + 2O2(g)  2NO2(g) ΔH1 = 68 kJ 2steps: N2(g) + O2(g)  NO(g) ΔH2 = 180 kJ 2NO(g) + O2(g)  2NO2(g) ΔH3 = –112 kJ Net rxn:

90 Ch6.3 – Hess’s Law In going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or a series of steps. 1 step: N2(g) + 2O2(g)  2NO2(g) ΔH1 = 68 kJ 2steps: N2(g) + O2(g)  NO(g) ΔH2 = 180 kJ 2NO(g) + O2(g)  2NO2(g) ΔH3 = –112 kJ Net rxn: N2(g) + 2O2(g)  2NO2(g) ΔH2 + ΔH3 = 68 kJ

91 C(s)diamond + O2(g)  CO2(g) ΔH = -396kJ
Ex1) Calculate ΔH for converting graphite to diamond, C(s)graphite  C(s)diamond using the enthalpies for combustion given: C(s)graphite + O2(g)  CO2(g) ΔH = -394kJ C(s)diamond + O2(g)  CO2(g) ΔH = -396kJ

92 2B(s) + 3/2O2(g)  B2O3(s) ΔH = –1273 kJ
Ex2) Calculate ΔH for the synthesis of diborane (B2H6), given the following reactions: 2B(s) + 3/2O2(g)  B2O3(s) ΔH = –1273 kJ B2H6(g) + 3O2(g)  B2O3(s) + 3H2O(g) ΔH = –2035 kJ H2(g) + ½O2(g)  H2O(l) ΔH = –286 kJ H2O(l)  H2O(g) ΔH = kJ

93 NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
HW#55) Given the following data: 2O3(g) → 3O2(g) ΔH = -427 kJ O2(g) → 2O(g) ΔH = +495 kJ NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ calculate ΔH for the reaction NO(g) + O(g) → NO2(g) Ch6 HW#7 p284 51,53,55,57

94 NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
HW#55) Given the following data: 2O3(g) → 3O2(g) ΔH = -427 kJ O2(g) → 2O(g) ΔH = +495 kJ NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ calculate ΔH for the reaction 2NO(g) + 2O3(g) → 2NO2(g) +2O2(g) ΔH = -398 kJ 3O2(g) → 2O3(g) ΔH = +427 kJ 2O(g) → O2(g) ΔH = -495 kJ 2NO(g) + 2O(g) → 2NO2(g) ΔH = -466 kJ NO(g) + O(g) → NO2(g) ΔH = -233 kJ Ch6 HW#7 p284 51,53,55,57

95 Ch6 HW#7 p284 51,53,55,57 51. The enthalpy of combustion of solid carbon to form carbon dioxide is kJ/mol carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is kJ/mol CO. Use these data to calculate ΔH for the reaction

96 Ch6 HW#7 p284 51,53,55,57 51. The enthalpy of combustion of solid carbon to form carbon dioxide is kJ/mol carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is kJ/mol CO. Use these data to calculate ΔH for the reaction 2C(s) + O2(g) → 2CO(g)

97 2CO2(g) → 2CO(g) + O2(g) ΔH = +566.6 kJ/mol
Ch6 HW#7 p284 51,53,55,57 51. The enthalpy of combustion of solid carbon to form carbon dioxide is kJ/mol carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is kJ/mol CO. Use these data to calculate ΔH for the reaction 2C(s) + O2(g) → 2CO(g) 2C(s) + 2O2(g) → 2CO2(g) ΔH = kJ/mol 2CO2(g) → 2CO(g) + O2(g) ΔH = kJ/mol 2C(s) + O2(g) → 2CO(g) ΔH = kJ/mol

98 2so2(g) + O2(g) → 2SO3(g) ΔH = -198.2 kJ
53. Given the following data: S(s) + 3/2O2(g) → SO3(g) ΔH = kJ 2so2(g) + O2(g) → 2SO3(g) ΔH = kJ calculate ΔH for the reaction S(s) + O2(g) → SO2(g)

99 2so2(g) + O2(g) → 2SO3(g) ΔH = -198.2 kJ
53. Given the following data: S(s) + 3/2O2(g) → SO3(g) ΔH = kJ 2so2(g) + O2(g) → 2SO3(g) ΔH = kJ calculate ΔH for the reaction S(s) + O2(g) → SO2(g) 2S(s) + 2(3/2O2(g)) → 2SO3(g) ΔH = kJ 2SO3(g) → 2so2(g) + O2(g) ΔH = kJ 2S(s) + 2O2(g) → 2SO2(g) ΔH = kJ S(s) + O2(g) → SO2(g) ΔH = kJ

100 H2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ
55. In class 57. Given the following data: H2(g) + 1/2O2(g) → H2O(l) ΔH = kJ N2O5(g) + H2O(l) → 2HNO3(l) ΔH = kJ 1/2N2(g) + 3/2O2(g) + 1/2H2(g) → HNO3(l) ΔH = kJ calculate the ΔH for the reaction 2N2(g) + 5O2(g) → 2N2O5(g)

101 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ
57. Given the following data: 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ 10(H2(g) + 1/2O2(g) → H2O(l)) ΔH=10(-285.8)kJ 2(2HNO3(l) → N2O5(g) + H2O(l)) ΔH =2(+76.6)kJ

102 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ
57. Given the following data: 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ 10(H2(g) + 1/2O2(g) → H2O(l)) ΔH=10(-285.8)kJ 2(2HNO3(l) → N2O5(g) + H2O(l)) ΔH =2(+76.6)kJ 2N2(g) + 6O2(g) + 2H2(g)→ 4HNO3(l) ΔH=-696.4kJ 10H2(g) + 5O2(g) → 10H2O(l) ΔH =-2858kJ 4HNO3(l) → 2N2O5(g) + 2H2O(l) ΔH =+153.2kJ 12H2(g) + 6O2(g) → 12H2O(l) + 2N2(g) + 5O2(g) → 2N2O5(g) ΔH = kJ total

103 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ
57. Given the following data: 4(1/2N2(g))+4(3/2O2(g))+4(1/2H2(g))→4(HNO3(l)) ΔH=4(-174.1)kJ 10(H2(g) + 1/2O2(g) → H2O(l)) ΔH=10(-285.8)kJ 2(2HNO3(l) → N2O5(g) + H2O(l)) ΔH =2(+76.6)kJ 2N2(g) + 6O2(g) + 2H2(g)→ 4HNO3(l) ΔH=-696.4kJ 10H2(g) + 5O2(g) → 10H2O(l) ΔH =-2858kJ 4HNO3(l) → 2N2O5(g) + 2H2O(l) ΔH =+153.2kJ 12H2(g) + 6O2(g) → 12H2O(l) + 2N2(g) + 5O2(g) → 2N2O5(g) ΔH = kJ total 12(H2O(l) → H2(g) + ½O2(g)) ΔH=12(+285.8)kJ 2N2(g) + 5O2(g) → 2N2O5(g) ΔH =-28.4kJ

104 Ch6.4 – Standard Enthalpies of Formation
C(s)graphite  C(s)diamond Enthalpy time

105 Standard Enthalpy of Formation (ΔHfo)
- change in enthalpy that accompanies the formation of 1 mole of a substance from its elements. (All substances in their standard states)

106 Standard Enthalpy of Formation (ΔHfo)
- change in enthalpy that accompanies the formation of 1 mole of a substance from its elements. (All substances in their standard states) - use the state of the substance as it exists at 1 atm and 25oC. Exs) oxygen: _____ sodium: ______ mercury: ______ - for gases use a pressure of 1 atm. - for solutions use a concentration of 1M.

107 Standard Enthalpy of Formation (ΔHfo)
- change in enthalpy that accompanies the formation of 1 mole of a substance from its elements. - use the state of the substance as it exists at 1 atm and 25oC. - for gases use a pressure of 1 atm. - for solutions use a concentration of 1M. - elements in their standard states = 0. - multiply # of moles to ΔH ΔHoreaction = ΣnpΔHfo(products) – Σnr Δhfo(reactants)

108 Ex1) Use the standard enthalpies of formation listed in Table6
Ex1) Use the standard enthalpies of formation listed in Table6.2 to calc the standard enthalpy change for the given reaction: 4NH3(g) + 7O2(g)  4NO2(g) + 6H2O(l)

109 Ex2) Use the standard enthalpies of formation listed in Table6
Ex2) Use the standard enthalpies of formation listed in Table6.2 to calc the standard enthalpy change for the given reaction: 2Al(s) + Fe2O3(s)  Al2O3(s) + 2Fe(s) Ch6 HW#8 p285 61,65,66 Ch6 Rev p283 28,35 (Go over B4 lab pt 1)

110 a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g)
Ch6 HW#8 p285 61,65,66 Ch6 Rev p283 28,35 (Go over B4 lab pt 1) 61. Use the values of ΔHfo in Appendix 4 to the calculate ΔHo for the following reactions. a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g) 2mol(-80kJ/mol)+ 3(0) + 2mol(-75kJ/mol) 2mol(135.1kJ/mol) + 6mol(-242kJ/mol) ΔHoreaction = (products) – (reactants)

111 a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g)
61. Use the values of ΔHfo in Appendix 4 to the calculate ΔHo for the following reactions. a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g) 2mol(-46kJ/mol)+ 3(0) + 2mol(-75kJ/mol) 2mol(135.1kJ/mol) + 6mol(-242kJ/mol) (-92kJ) + (-150kJ) (270kJ) + (-1452kJ) (-242kJ) (-1182kJ) ΔHoreaction = (-1182kJ)– (-242kJ) = -940kJ

112 ΔHoreaction = (products) – (reactants)
61 - b. Ca(PO4)2(s) + 3H2SO4(l) → 3CaSO4(s) + 2H3PO4(l) 1mol(-4126kJ/mol) + 3mol(-814kJ/mol) 3mol(1433kJ/mol)+2mol(-1267kJ/mol) ΔHoreaction = (products) – (reactants)

113 (-4126kJ) + (-2442kJ) (-4299kJ) + (-2534kJ)
61 - b. Ca(PO4)2(s) + 3H2SO4(l) → 3CaSO4(s) + 2H3PO4(l) 1mol(-4126kJ/mol) + 3mol(-814kJ/mol) 3mol(-1433kJ/mol)+2mol(-1267kJ/mol) (-4126kJ) + (-2442kJ) (-4299kJ) + (-2534kJ) (-6568kJ) (-6833kJ) ΔHoreaction = (products) – (reactants) ΔHoreaction = (-6833kJ)– (-6568kJ) = -265kJ

114 61 - c. NH3(g) + HCl(g) → NH4Cl(s)
1mol(-46kJ/mol) + 1mol(-92kJ/mol) 1mol(-314kJ/mol) ΔHoreaction = (products) – (reactants)

115 ΔHoreaction = (products) – (reactants)
61 - c NH3(g) + HCl(g) → NH4Cl(s) 1mol(-46kJ/mol) + 1mol(-92kJ/mol) 1mol(-314kJ/mol) (-46kJ) + (-92kJ) (-314kJ) (-138kJ) (-314kJ) ΔHoreaction = (products) – (reactants) ΔHoreaction = (-314kJ)– (-138kJ) = -176kJ

116 3Al(s) + 3NH4ClO4(s)→Al2O3(s) + AlCl3(s) + NO(g) +6H2O(g)
65. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is Calculate the ΔHo for this reaction. 3Al(s) + 3NH4ClO4(s)→Al2O3(s) + AlCl3(s) + NO(g) +6H2O(g) 3(0) mol(-295kJ/mol) 1mol(-1676)+1mol(-704)+1mol(90)+6(-242) ΔHoreaction = (products) – (reactants) ΔHoreaction =

117 3Al(s) + 3NH4ClO4(s)→Al2O3(s) + AlCl3(s) + NO(g) +6H2O(g)
65. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is Calculate the ΔHo for this reaction. 3Al(s) + 3NH4ClO4(s)→Al2O3(s) + AlCl3(s) + NO(g) +6H2O(g) 3(0) mol(-295kJ/mol) 1mol(-1676)+1mol(-704)+1mol(90)+6(-242) (-885kJ) (-1676kJ) + (-704kJ) + (+90) + (-1452) (-885kJ) (-3742kJ) ΔHoreaction = (products) – (reactants) ΔHoreaction = (-3742kJ)– (-885kJ) = -2857kJ exothermic

118 4N2H3CH3(l) + 5N2O4(l) → 12H2O(g) + 9N2(g) + 4CO2(g)
66. The space shuttle orbiter utilizes the oxidation of methyl hydrazine by dinitrogen tetroxide for propulsion: Calculate the ΔHo for this reaction. 4N2H3CH3(l) + 5N2O4(l) → 12H2O(g) + 9N2(g) + 4CO2(g) 4(54) (-20) (-242) (0) (-393.5) ΔHoreaction = (products) – (reactants)

119 4N2H3CH3(l) + 5N2O4(l) → 12H2O(g) + 9N2(g) + 4CO2(g)
66. The space shuttle orbiter utilizes the oxidation of methyl hydrazine by dinitrogen tetroxide for propulsion: Calculate the ΔHo for this reaction. 4N2H3CH3(l) + 5N2O4(l) → 12H2O(g) + 9N2(g) + 4CO2(g) 4(54) (-20) (-242) (0) (-393.5) (+116kJ) (-4478kJ) ΔHoreaction = (products) – (reactants) ΔHoreaction = (-4478kJ)– (+116kJ) = -4594kJ very exothermic! Do u think that might be a very powerful and very spontaneous reaction?!? Where does all the energy come from?

120 Ch6 Rev p283 28,35,46,54,64 28. One mole of H2O(g) at 1.00atm and 100°C occupies a volume of 30.6L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00atm and 100°C, 40.66kJ of heat is released. If the density of H2O(l) at the this temp and pressure is g/cm3, calc ∆E for the condensation of one mole of of H2O. H2O(g) H2O(l) 1mol d= 0.996g/cm3 V=30.6L P=1atm T=100°C ∆E =?

121 ∆E = q + W work done on system ∆E = q + (-P.∆V)
28. One mole of H2O(g) at 1.00atm and 100°C occupies a volume of 30.6L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00atm and 100°C, 40.66kJ of heat is released. If the density of H2O(l) at the this temp and pressure is g/cm3, calc ∆E for the condensation of one mole of of H2O. H2O(g) H2O(l) kJ 1mol 1mol V=30.6L d= 0.996g/cm3 ΔH  q P=1atm T=100°C ∆E =? ∆E = q + W work done on system ∆E = q (-P.∆V) ∆E = (-40.66kJ) + (101.3kPa) .∆V

122 ∆E = q + W work done on system ∆E = q + (-P.∆V)
28. One mole of H2O(g) at 1.00atm and 100°C occupies a volume of 30.6L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00atm and 100°C, 40.66kJ of heat is released. If the density of H2O(l) at the this temp and pressure is g/cm3, calc ∆E for the condensation of one mole of of H2O. H2O(g) H2O(l) kJ 1mol 1mol V=30.6L d= 0.996g/cm3 q P=1atm T=100°C ∆E =? ∆V = 0.018L – 30.6L = L ∆E = q + W work done on system ∆E = q (-P.∆V) ∆E = (-40.66kJ) + (101.3kPa) .∆V

123 ∆E = q + W work done on system ∆E = q + (-P.∆V)
28. One mole of H2O(g) at 1.00atm and 100°C occupies a volume of 30.6L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00atm and 100°C, 40.66kJ of heat is released. If the density of H2O(l) at the this temp and pressure is g/cm3, calc ∆E for the condensation of one mole of of H2O. H2O(g) H2O(l) kJ 1mol 1mol V=30.6L d= 0.996g/cm3 q P=1atm T=100°C ∆E =? ∆V = 0.018L – 30.6L = L ∆E = q + W work done on system ∆E = q (-P.∆V) ∆E = (-40.66kJ) + (-(101.3kPa) .∆V) ∆E = (-40.66kJ) + (-(101.3kPa) .(-30.58L)) ∆E = kJ + (+3.097kJ) = kJ

124 C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) + 1.3x108J
35. Consider the combustion of propane: C3H8(g) + 5O2(g) CO2(g) + 4H2O(l) + 1.3x108J Assume that all the heat in sample Exercise 6.3 comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 60% efficient? 1.3x108J (from 6.3) 60% efficient means you gotta burn a whole lot more  1.3x108J / 0.60 = 2.17x108J will get you there.

125 C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) + 1.3x108J
35. Consider the combustion of propane: C3H8(g) + 5O2(g) CO2(g) + 4H2O(l) + 1.3x108J ?g

126 Heat absorbed by ammonium nitrate, comes from the soln,
Rev – Day 2 (Lab6.2 Day 2) 46. In a coffee-cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.00oC. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34o C. Assuming the solution has a heat capacity of 4.18 J/oC.g and assuming that no heat loss to the calorimeter. Calculate the enthalpy charge for the dissolution of NH4NO3 in units of kJ/mol . NH4NO water NH NO3- m=1.60g m=75.0g ∆H = ? (kJ/mol) Ti = 25.00C Ti = 25.00C Tf = 23.34C Tf = 23.34C Heat absorbed by ammonium nitrate, comes from the soln, and is measured in the temp change of the total soln: q = – m.cp.ΔT

127 Heat absorbed by ammonium nitrate, comes from the soln,
46. NH4NO water NH NO3- m=1.60g m=75.0g Ti = 25.00C Ti = 25.00C Tf = 23.34C Tf = 23.34C Heat absorbed by ammonium nitrate, comes from the soln, and is measured in the temp change of the total soln : q = – m.cp.ΔT

128 When 1.60g NH4NO3 dissolved, 532 J (q) was released.
46. NH4NO3 +____ water NH NO3- m=1.60g m=75.0g Ti = 25.00C Ti = 25.00C Tf = 23.34C Tf = 23.34C Heat absorbed by ammonium nitrate, comes from the soln, and is measured in the temp change of the total soln : q = – m.cp.ΔT When 1.60g NH4NO3 dissolved, 532 J (q) was released. How much heat (ΔH) would 1 mol produce?

129 When 1.60g NH4NO3 dissolved, 532 J (q) was released.
46. NH4NO kJ water NH NO3- m=1.60g m=75.0g Ti = 25.00C Ti = 25.00C Tf = 23.34C Tf = 23.34C Heat absorbed by ammonium nitrate, comes from the soln, and is measured in the temp change of the total soln : q = – m.cp.ΔT When 1.60g NH4NO3 dissolved, 532 J (q) was released. How much heat (ΔH) would 1 mol produce?

130 C2H2(g) + 5/2O2(g) 2CO2(g) + H20(l) ∆H= -1300kJ
54. Given the following data: C2H2(g) + 5/2O2(g) CO2(g) + H20(l) ∆H= -1300kJ C(s) + ½O2(g) CO2(g) ∆H= -394kJ H2 (g) + ½O2(g) H2O(l) ∆H= -286kJ Calculate ∆H for the reaction: 2C (s) + H2 (g) C2H2 (g)

131 64.Calculate ∆H˚ for each of the following reactions using the data provided:
2Na(s)+2H2O(l) → 2NaOH(aq)+H2(g) 2Na(s)+CO2(g) → Na2O(s)+CO(g)


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