1. UNIT 3 Review How can energy changes be represented in chemical reactions? Thermochemical equations with energy term beside the equation e.g. N 2 (g) + 2O 2 (g) → 2NO 2 (g) ΔH r = +66.4 kJ Thermochemical equations with energy term as product or reactants e.g. N2(g) + 2O2(g) + 66.4 kJ → 2NO2(g) Enthalpy diagrams

2. UNIT 3 Section 5.2 What to use when Chapter 5: Energy Changes When the problem is about: A solid dropped into water (like the copper penny expt): Use: Q released = Q gained where Q= mc∆T If it is as above but the container c and m is given use: Q released by reaction = Q gained by water + Q gained by container If the question is asking for molar enthalpy of reaction, and gives c and m, then calculate Q first (which is ∆H) and then use ∆H = n∆H  If it is about enthalpy in aqueous solutions, use C= n/V and if as above it is a solid and molar enthalpy is needed, then you need: n=m/M

3. UNIT 3 Section 5.3 Hess’s Law - calculating the enthalpy change of reactions using existing data - When using calorimetry is impractical The enthalpy change of any reaction can be determined if: the enthalpy changes of a set of reactions “add up to” the overall reaction of interest standard enthalpy change, ΔH°, values are used

4. UNIT 3 Section 5.3 For example Chapter 5: Energy Changes To find the enthalpy change for formation of SO 3 from O 2 and S 8, you can use

5. UNIT 3 Section 5.3 Techniques for Manipulating Equations 1.You can reverse an equation the products become the reactants, and reactants become the products the sign of the ΔH value must be changed 2.You can multiply each coefficient all coefficients in an equation are multiplied by the same integer or fraction the value of ΔH must also be multiplied by the same number

6. UNIT 3 Section 5.3 Standard Molar Enthalpies of Formation Chapter 5: Energy Changes Often used for Hess’ Law is standard molar enthalpy of formation, ΔH˚ f the change in enthalpy when 1 mol of a compound is synthesized from its elements in their most stable form at SATP conditions enthalpies of formation for elements in their most stable state under SATP conditions are set at zero since formation equations are for 1 mol of compound, many equations include fractions (for a balanced eq’n)

7. UNIT 3 Section 5.3 Formation Reactions and Thermal Stability Chapter 5: Energy Changes The thermal stability of a substance is the ability of the substance to resist decomposition when heated. decomposition is the reverse of formation the opposite sign of an enthalpy change of formation for a compound is the enthalpy change for its decomposition the greater the enthalpy change for the decomposition of a substance, the greater the thermal stability of the substance

8. UNIT 3 Section 5.3 Using Enthalpies of Formation and Hess’s Law Chapter 5: Energy Changes So the enthalpy of a reaction = the sum of all the products – the sum of all the reactants. For example: CH 4 (g) + 2O 2 (g) → CO 2 (g) + 2H 2 O(g)

9. Determine ∆H˚ r for the following reaction using the enthalpies of formation that are provided. UNIT 3 Section 5.3 C 2 H 5 OH(l) + 3O 2 (g) → 2CO 2 (g) + 3H 2 O(l) ∆H˚ f of C 2 H 5 OH(l): –277.6 kJ/mol ∆H˚ f of CO 2 (g): –393.5 kJ/mol ∆H˚ f of H 2 O(l): –285.8 kJ/mol T RY THIS

10. ∆ H ˚ r = [(2 mol)( ∆ H˚ f CO 2 (g)) + (3 mol)( ∆ H˚ f H 2 O(l))] – [(1 mol)(∆H˚ f C 2 H 5 OH(l)) + (3 mol)(∆H˚ f O 2 (g)] Section 5.3 UNIT 3 Chapter 5: Energy Changes ∆ H ˚ r = [(2 mol)(–393.5 kJ/mol) + (3 mol)(–285.8 kJ/mol)] – [(1 mol)(–277.6 kJ/mol) + (3 mol)(0 kJ/mol)] ∆ H ˚ r = (–1644.4 kJ) – (–277.6 kJ) ∆H˚ r = –1366.8 kJ

11. UNIT 3 Section 5.4 5.4 Energy Efficiency and Energy Resources Chapter 5: Energy Changes Energy efficiency can be calculated using the equation:

12. UNIT 3 Section 5.4 Using Energy Efficiently TO PREVIOUS SLIDEPREVIOUS Chapter 5: Energy Changes Energy use distribution in Canadian homes A challenge in the development of energy efficient technology is to find ways to best convert energy input into useful forms. For example, efficiency of appliances: conversion of input of electrical energy versus output of energy usually all that is considered but should also consider efficiency of the source of the electricity

13. UNIT 3 Section 5.4 Conventional Energy Sources in Ontario TO PREVIOUS SLIDEPREVIOUS Chapter 5: Energy Changes The distribution of energy sources in Ontario The three main sources of electrical energy in Ontario: nuclear power plants power plants that burn fossil fuels (natural gas and coal) hydroelectric generating stations

14. UNIT 3 Section 5.4 Alternative Renewable Energy Sources in Ontario TO PREVIOUS SLIDEPREVIOUS Chapter 5: Energy Changes Renewable energy sources in Ontario: account for about 25% of energy production are projected to increase to as high as 40% by 2025 include hydroelectric power (major source), wind energy (currently ~ 1% and projected to 15% in 2025), and solar energy (currently low but may be as high as 5% in 2025). Much lower contributors are biomass, wave power, and geothermal energy.

15. UNIT 3 Section 5.4 What Is a “Clean” Fuel? TO PREVIOUS SLIDEPREVIOUS Chapter 5: Energy Changes Different fuels have differing impacts on the environment. One way this impact is measured is through emissions. For example, CO 2 (g) emissions per kJ of energy produced. Fuelkg CO 2 / kJ energy Anthracite coal108.83 Oil78.48 Natural gas56.03 Nuclear0.00 Renewables0.00