Thermodynamics and Kinetics Guided Notes
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This document contains guided notes on thermodynamics and kinetics for a chemistry unit. It defines key concepts like energy, heat, temperature, enthalpy, entropy, Gibbs free energy, and specific heat. It explains endothermic and exothermic reactions, Hess's law, and how to calculate heat transfer using specific heat capacity. Sample problems are provided to demonstrate calculating heat and temperature changes. The document is a set of lecture notes intended to instruct students on important topics in thermodynamics.
Thermodynamics and Kinetics Guided Notes
- 1. Chemistry Guided Notes Unit 5: Thermodynamics and Kinetics Name: Date: Period: object Energy What is Energy? • Energy‐ • Chemical Potential Energy‐ of atoms of atoms of bonds object to a What is Heat? • Heat (q)‐ • Heat always flows from a Warmer object losses energy in the form of heat and its temperature Cooler object gains energy in the form of heat and its temperature • NOT THE SAME AS TEMPERATURE • Temperature (T)‐ • Measuring Heat: Two Units Calorie (cal)‐ Joule (J)‐ Thermochemistry and Enthalpy Thermochemistry • Thermochemistry‐ • Universe= System + Surroundings System‐ Surroundings‐ Enthalpy (H) • Enthalpy (H)‐ • Enthalpy of a Reaction (ΔHrxn)= • Thermochemical equation are balanced equations that include values for ΔHrxn Endothermic Reactions • • • Exothermic Reactions
- 2. • • • Hess’s Law • Hess’s Law‐ states that if you can add two or more thermochemical reaction equations to produce a final equation for the reaction then the sum of the enthalpy changes for the individual reactions is the enthalpy change for the final reaction • Three Rules: If the reaction must be doubled, If the reaction must be reversed, Anything on both sides of the final equation can be • Example: Calculate the ΔH for the reaction 2S (s) + 3 O2 → 2SO3 (g) using the information below. a. 2SO3 (g) → 2SO2 (g) + O2 (g) ΔH= 198 kJ b. S (s) + O2 → SO2 (g) ΔH= ‐297kJ SO3 is on the product side of the desired equation so reverse reaction a. The coefficient of the 1st reactant, S (s) is 2 in the desired equation. Therefore, reaction b must be doubled. Add the equations together and cancel anything that occurs on both the reactant and product side. Write the final equation for the reaction including the ΔH value. Box or Circle. Spontaneity, Entropy, Enthalpy, and Gibb’s Free Energy
- 3. Spontaneity • Spontaneous Processes‐ • Nonspontaneous Processes‐ Entropy (S) • Entropy (S)‐ • 2nd Law of thermodynamics‐ Gibb’s Free Energy (G) • Gibb’s Free Energy (G)‐ • Relates and can be used to predict reaction spontaneity • Formula for Gibb’s Free Energy: and • If ΔG value is negative, If ΔG value is positive, Spontaneity, Enthalpy, and Entropy Exothermic Reaction (ΔH) Endothermic Reaction (+ΔH) Increased Entropy (+ΔS) Decreased Entropy (ΔS) Specific Heat Specific Heat (c) • Specific Heat (c)‐ • • Substances with high specific heat • Substances with low specific heat
- 4. • Formula for Calculating Heat Released or Absorbed: • if the value for q is negative, • q‐ if the value for q is positive, m‐ c‐ ΔT‐ must be absorbed by the Law of Conservation of Energy • Law of Conservation of Energy‐ • 1st Law of Thermodynamics • Heat lost by the • Heat transfer is measured using a device called a calorimeter Specific Heat Example Problems • • Example 1: Calculating Heat‐ If the temperature of 34.4g of ethanol increases from 25.0°C to 78.8°C, how much heat has been absorbed by the ethanol? (The specific heat of ethanol is 2.44J/g°C) Example 2: Calculating Temperature‐ A 4.50g nugget of pure gold absorbed 267J of heat. What was the final temperature of the gold if the initial temperature was 25°C? (The specific heat of gold is 0.129J/g°C.)
- 5. • Example 3: Calculating Specific Heat‐ A 155g sample of an unknown substance was heated from 25.0°C to 40.0°C. In the process, the substance absorbed 5696 J of energy. What is the specific heat of the substance? Activation Energy and Reaction Rates Reaction Energy Diagrams Reaction Progress Reaction Progress Activation Energy Activation Energy (EA)‐ • • Reaching the activated complex requires • High activation energy correlates to a • Low activation energy correlates to a Factors that Affect Reaction Rates • Nature of Reactants‐ • Concentration‐ • Surface Area‐ • Temperature‐ Catalyst‐ •