Presentation on theme: "Unit 1 – Thermochemistry"— Presentation transcript:
1Unit 1 – Thermochemistry General Outcomes:Determine and interpret energy changes in chemical reactionsExplain and communicate energy changes in chemical reactions
2Key Concepts Enthalpy of formation Enthalpy of reaction ΔH notation Hess’ LawMolar enthalpyEnergy diagramsActivation EnergyCatalystsCalorimetryFuels and Energy Efficiency
3Energy the potential to do work. examples of energy changes: - chemical energy in food to motion- solar energy to power- geothermal energy to heat- nuclear energy to power, heat, motion
4Thermodynamics: study of energy changes in systems Thermochemistry –study of energy changes involved in physical and chemical changes.
5Laws of Thermodynamics First Law - Energy can be neither created nor destroyed, it simply changes forms. Esystem = -Esurroundings Second Law – In any energy conversion, energy is always lost in the form of heat.
6How do we know energy changes exist? We can observe the effect it has on our surroundings.Energy systems either release energy to the surroundings or absorb energy from the surroundings.Universe = System + Surroundings
10Calculating Thermal Energy Q=mcΔT YouTube - Chemistry Music Video: Em Cee Delta Tee (The Calorimetry Song)
11Q =quantity of heat flowing in / out of that substance, measured as energy in units of joules (J) or kilojoules (kJ)m-mass of substance undergoing the change measured in units of grams (g) or kilograms (kg)c=heat capacity -heat required to change the temp of 1 g of substance by 1oC
12Example Calculations (Q=mcΔT) Many hot water heaters use the combustion of natural gas to heat the water in the tank. When 150 L of water at 10oC is heated to 65oC, how much energy flows into the water?
13A solid substance has a mass of 250. 0 g. It is cooled by 25 A solid substance has a mass of g. It is cooled by 25.0oC, and loses kJ of heat. What is the specific heat capacity and the identity of the substance?
14If a copper pot weighing 0. 500 kg is heated with 2 If a copper pot weighing kg is heated with kJ of energy, what is the expected temperature change?
15Energy From the SunEnergy from the sun is stored in the bonds of chemical substances such as fossil fuels and hydrocarbons.
16Solar energy is captured by plants during photosynthesis. Living tissues from plants and animals become buried. Instead of decaying, these compounds form hydrocarbons or fossil fuels.The energy from fossil fuels is released during combustion reactions and converted into heat.
17Photosynthesis is endothermic: 6CO2(g) + 6H2O(l) + energy C6H12O6(s) + 6O2(g)Cellular Respiration is exothermic:C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l) + energyCombustion is exothermic:CH4(g) O2(g) CO2(g) H2O(g) + energy
19There are two types of energy that matter may possess: Energy TypesThere are two types of energy that matter may possess:1. Kinetic energy – the energy of motion2. Potential energy – the energy of position
20Kinetic Energy (Ek)faster the particle is moving, the greater the kinetic energy.Can be found in three types:TranslationalRotationalVibrational
21Ek measured indirectly by measuring the temperature of a system. is proportional to the amount of heat a system holds.
22Potential Energy (Ep)Stored energy found in the bonds and inter-molecular forces of moleculesChanges in potential energy include phase changes, chemical reactions and nuclear reactions
23Chemical Changes Are changes in potential energy energy is required to break bonds and the energy is released when new bonds are formed.chemical reactions:micro/macro
24Enthalpy and Enthalpy Change enthalpy describes the total amount of energy a system has.Enthalpy Change (ΔH = kJ) refers to how much the total energy of a system increases or decreases during a chemical reaction.Molar enthalpy (ΔH = kJ/mol) describes the amount of enthalpy change per mole of substance.
25Two types of reaction enthalpies Exothermic reaction – more energy is released in making bonds than is required to break them.(-ΔH)Surrounding temperature increasesEndothermic reaction – less energy is released in forming bonds than was required to break bonds.(+ΔH)Surrounding temperature decreases
27Calculating enthalpy changes H = n H H = change in enthalpy (kJ) H = molar enthalpy kJ/mol n = moles n=m/M
28Example Calculations ΔH = nH Hydrogen and oxygen gas react to produce g of water vapor. If the molar enthalpy of reaction is kJ/mol for water, what is the enthalpy change?
29The molar enthalpy of combustion for ethanol is -725. 9 kJ/mol The molar enthalpy of combustion for ethanol is kJ/mol. What mass of methanol must be burned to generate 2.34 x 104 kJ of energy?
30What is the molar enthalpy of combustion if a 10 What is the molar enthalpy of combustion if a 10.0 g sample of pure acetic acid is burned in oxygen and produces kJ of energy?
31Expressing Enthalpy Change 1. Molar enthalpy of a specific reaction relative to one species in the reaction.2H2(g) + O2(g) 2H2O(g) H: kJ/mol H2O2. Enthalpy change for a balanced reaction equation.2H2(g) + O2(g) 2H2O(g) ∆H: kJ
323. Including the energy value as part of the balanced equation. 2H2(g) + O2(g) 2H2O(g) kJ2C(g) + 2H2(g) kJ C2H4(g)4. Drawing a potential energy diagram for the reaction.
34Calorimetryused to determine energy changes during physical or chemical processescalorimeter : ideally an isolated systemEnergy in Chemical Reactions - Learning Activit - Flash Player Installation
35Mathematically, calorimetry may be described as: All components of the calorimeter are included in the total energy change.Mathematically, calorimetry may be described as:Heat lost = heat gained(* remember heat lost is expressed as a negative value)
36Simple Calorimeter used for reactions in aqueous solution can calculate the heat change in the water and use to determine enthalpy changeP 353 lists assumptions made when using a simple calorimeter
38Example Questions50.00mL of 0.300mol/L CuSO4(aq) is mixed with 50.00mL of NaOH(aq). The initial temperature of both solutions is oC and the highest temperature recorded after mixing is 24.60oC.Determine the enthalpy change for the systemDetermine the molar enthalpy change for CuSO4Write the thermochemical equation.
39Barium chloride and sodium sulfate react to produce a precipitate of barium sulfate. When mol of precipitate is formed the temperature of 3.00 kg of water is raised from to oC. Calculate the molar enthalpy of reaction for the production of barium sulphate.
40Bomb Calorimeterused for combustion reactionstotal energy change of the calorimeter includes changes in the container itself, the water, the thermometer and the stirrer.
41bomb calorimeters may report a heat capacity for the entire calorimeter system. (C measured in J/oC) Q = CT
42Example CalculationsA bomb calorimeter has a heat capacity of 40.00kJ/oC. Complete combustion of 1.00g of hydrogen causes the temperature of the calorimeter to increase by 3.54oC. What is the molar enthalpy of combustion from this evidence?
43When 1. 00 g of propane is burned, about 2. 36 J of heat is given off When 1.00 g of propane is burned, about 2.36 J of heat is given off. What mass of water at 50.0oC can be heated to 80oC when 4.00 mol of propane is burned?
44A strip of magnesium metal having a mass of 1 A strip of magnesium metal having a mass of 1.22 g is placed in 100 mL of mol/L HCl(aq) in a metal can with a heat capacity of 562 J/oC. After the reaction, the temperature increased from 23.0oC to 45.5oC. Assuming the solution in the calorimeter has the same heat capacity as water, determine the heat of reaction per mole of magnesium.