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Chpt 6 - Thermochemistry Energy and framework (definitions) Internal energy, heat & work Enthalpy & Calorimetry Hesss Law Standard Enthalpies Applications?

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Presentation on theme: "Chpt 6 - Thermochemistry Energy and framework (definitions) Internal energy, heat & work Enthalpy & Calorimetry Hesss Law Standard Enthalpies Applications?"— Presentation transcript:

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2 Chpt 6 - Thermochemistry Energy and framework (definitions) Internal energy, heat & work Enthalpy & Calorimetry Hesss Law Standard Enthalpies Applications? HW: Chpt 6 - pg , #s 14, 16, 24, 27, 28, 32, 34, 38, 41, 42, 44, 49, 54, 62, 72, 73, 80, 84, 112 Due Wed Oct. 7

3 Thermodynamic Framework Energy - capacity to do work or produce heat Law of conservation of energy PE (generally chemical potential energy) and KE Heat involves a transfer of energy - Very different from temperature (a measure of motions of particles) Heat is NOT a substance Work is force acting over a distance

4 State Functions Energy = work + heat –Ball rolling down hill example - heat and work are different depending on pathway

5 State Functions - cont State function or state property only depends on current state not pathway –Energy is state function –Heat and work are not state functions –Another example, Elevation vs. Distance

6 Chemical Energy System and surroundings Exothermic and endothermic –Chemical PE thermal energy Recall energy reaction diagrams –Only concerned with Energy of Reactants and Products (not pathway) Internal Energy E = q + wq=heat, w=work 1st Law of thermodynamics –Energy of Universe is constant

7 Universe Energy is Constant Exothermic or Endothermic?

8 Chemical Energy - cont Quantities have sign and magnitude –Systems perspective for sign, thus endo is flow into system so q is positive (gaining heat) – E 0 endothermic –Work done on system is positive, w>0 –Work done by system is negative, w<0

9 PV Work Common types of work are expansion by a gas and compression on a gas PV work, w = - P V if volume is expanding w = P V if volume is compressing V = V final - V initial,

10 PV Work - derivation Example that shows Pressure=force/area = F/A so F = P x A Work is force x dist = F x h so W = P x A x h volume of cylinder = A x h Thus W = P V The sign is (-) for expanding gas, since work is done by system on surroundings

11 Enthalpy, H H = E + PV, since E, P and V are state functions H is also a state function At constant pressure H = q p (q p is heat at const p) In general, for open laboratory chemical reactions pressure is constant, so the change in enthalpy is used interchangeably with the heat of a reaction. For a chemical reaction H = H products - H reactants Exothermic means enthalpy, H < 0 Endothermic means enthalpy, H > 0

12 Calorimetry The science of measuring heat. Substances absorb heat differently; heat capacity, C, measures this C = heat absorbed / increase in temp Specific heat capacity is per gram substance A calorimeter measures heat change. q = C x m x T our text uses s for C The AP test will use C, actually C p

13 Calorimeter Simple styrofoam cup calorimeter is easily used for lab measurements and constant pressure measurements.

14 Bomb Calorimeter A Bomb calorimeter schematic - it only looks like a bomb. It is used when constant volume measurements are needed.

15 Hesss Law Since enthalpy is a state function, heat of reactions can be calculated from a known set of simple chemical rxns combined together to get the final rxn. One step: N 2 (g) + 2O 2 (g) --> 2NO 2 (g) H = 68kJ Two distinct steps N 2 (g) + O 2 (g) --> 2NO(g) H = 180kJ 2NO(g) + O 2 (g) --> 2NO 2 (g) H = -112kJ Total these reactions N 2 (g) + 2O 2 (g) --> 2NO 2 (g) H = 68kJ

16 Hesss Law schematic The overall reaction enthalpy is independent of pathway

17 Hesss Law rules Characteristics of H for a rxn If a reaction is reversed, the sign of H is also reversed. The magnitude of H is directly proportional to the quantities of reactants and products in the rxn –i.e. if the coefficients are multiplied by an integer, H is multiplied by same integer.

18 Example 6.8 pg. 254 We want to calculate the H for the synthesis of diborane, B 2 H 6, from its elements. 2B(s) + 3H 2 (g) --> B 2 H 6 (g) H = ? Use the following data: 2B(s) + 3/2O 2 (g) --> B 2 O 3 (s) H = kJ B 2 H 6 (g) + 3O 2 (g) --> B 2 O 3 (s) +3H 2 O(g) H = kJ H 2 (g) + 1/2O 2 (g) --> H 2 O(l) H = -286 kJ H 2 O(l) --> H 2 O(g) H = 44 kJ Hints - 1) work backward from the required/desired reaction, 2) reverse any reaction as needed to align reactants and products, 3)multiply any reaction as necessary to get correct coefficients. Recall H is a state function (independent of pathway)

19 Standard Enthalpies of Formation H f o of a substance is the change in enthalpy that accompanies the formation of 1 mole of the substance from its elements in their standard states. Standard state: gas is 1 atm, liquid or solid is pure substance, solutions are 1M. Elements are state at 1atm and 25 o C.

20 Calculating H from H f o Since enthalpies are state functions independent of pathway, in chemical reactions, the reactants can be taken apart into their elements and the products can be constructed from their elements. For a chemical reaction H = n p H f o (products) - n r H f o (reactants) Data found in Appendix 4 - pg A19 - A22

21 Example H from H f o 4 NH 3 (g) (g) --> 4 NO 2 (g) + 6 H 2 O(l) NH 3 (g) -46 kJ/molNO 2 (g) 34kJ/mol H 2 O(l) -286kJ/molO 2 (g)0 kJ/mol H = Products - Reactants… 4x34kJ/mol + 6x(-286kJ/mol) x(-46kJ/mol) H = -1396kJ/mol

22 Greenhouse Effect


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