Chapter 6 - Thermochemistry

Section 6.1 The Nature of Energy

• Energy• Law of Conservation of Energy• Potential energy• Kinetic energy• Heat • Work• Pathway• State function or property• Chemical Energy

Chemical Energy

• System• Surroundings• Exothermic• Endothermic• Thermodynamics• First Law of Thermodynamics• Internal energy• Problems – pages 246 - 248

Section 6.2 Enthalpy and Calorimetry• Enthalpy

ΔH = Hproducts – Hreactants

• Sample problems – page 249 – 250• Calorimetry

q = c x m ΔT

• Specific heat capacity• Molar heat capacity• Constant-pressure calorimetry• Problems page 251 – 256

Section 6.3 Hess’s Law

• Hess’s Law

• Characteristics of Enthalpy changes1. If a reaction is reversed, the sign of ΔH is

also reversed.

2. The magnitude of ΔH is directly proportional to the quantities of reactants and products in a reaction.

• Problems pages 258 - 259

Section 6.4 Standard Enthalpies of Formation

• Standard enthalpy of formation

• Standard state

• Definitions of Standard StatesFor a compound– The standard state of a gaseous substance is a

pressure of exactly 1atm– For a pure substance in a condensed state (solid or

liquid), the standard state is the pure liquid or solid– For a substance present in a solution, the standard

state is a concentration of exactly 1M.

For an element– The standard state of an element is the form in which

the element exists under conditions of 1 atm and 25°C. (The standard state for oxygen is O2(g) at a pressure of 1 atm; the standard state for sodium is Na(s); the standard state for mercury is Hg(l).

Calculating Enthalpy Changes

ΔH°reaction =∑np ΔH°f(products) - ∑np ΔH°f(reactants)

Problems pages 263 – 267Reminders:

* When a reaction is reversed, the magnitude of ΔH remains the same, but its sign changes.* When the balanced equation for a reaction is multiplied by an integer, the value of ΔH must be multiplied by the same integer.* Elements in their standard states are not included in ΔH°reaction calculations.