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AHvaforization = 2260 J/g your ne valadies gniwotlot de 2 by 01 Practice Problems 1. A copper pot with a mass of 772 grams absorbs 22.7 kJ of heat. Its final temperature is 137 °C. What was its initial temperature? 2. How much heat is absorbed by a 15.5 g piece of gold as it is heated from 4.5 °C to 177.4°C? 3. A container full of water absorbs 64.4 kJ of heat and its temperature rises from 22.0 °C to 73.4 °C. What is the volume of water in mL? (The density of water is 1 g/mL) the brown gas

AHvaforization = 2260 J/g your ne valadies gniwotlot de 2 by 01 Practice Problems 1. A copper pot with a mass of 772 grams absorbs 22.7 kJ of heat. Its final temperature is 137 °C. What was its initial temperature? 2. How much heat is absorbed by a 15.5 g piece of gold as it is heated from 4.5 °C to 177.4°C? 3. A container full of water absorbs 64.4 kJ of heat and its temperature rises from 22.0 °C to 73.4 °C. What is the volume of water in mL? (The density of water is 1 g/mL) the brown gas

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Hi sorry to bother I know that you guys can only answer 3 questions per the ask questions so I was wondering if you could solve the following 3 for me please thank you
--- ### Unit 5 Study Guide #### Topics Covered: - Exothermic vs. Endothermic Reactions - Measuring Heat Flow (Specific Heat Capacity) - Enthalpy, Entropy, Gibbs Free Energy - Heats of Formation - Thermochemical Equations - Spontaneity of Reactions #### Equations: 1. **q = mCΔT** 2. **ΔH = ΣnΔH (products) - ΣnΔH (reactants)** 3. **ΔH_fusion = 334 J/g** 4. **ΔH_vaporization = 2260 J/g** 5. **q = mΔH_fusion** 6. **ΔG = ΣnΔG (products) - ΣnΔG (reactants)** 7. **q = mΔH_vaporization** 8. **ΔS = ΣnΔS (products) - ΣnΔS (reactants)** 9. **ΔG = ΔH - TΔS** #### Constants: - **C_water** = 4.184 J/g°C - **C_iron** = 0.449 J/g°C - **C_copper** = 0.385 J/g°C - **C_steam** = 2.03 J/g°C - **ΔH_fusion** = 334 J/g - **ΔH_vaporization** = 2260 J/g #### Practice Problems: 1. **A copper pot with a mass of 772 grams absorbs 2450 J of heat. Its final temperature is 137°C. What was its initial temperature?** 2. **How much heat is absorbed by a 15.5 g piece of gold as it is heated from 4.5°C to 177.4°C?** 3. **A container full of water absorbs 64.4 kJ of heat, and its temperature rises from 22.0°C to 73.4°C. What is the volume of water in mL? (The density of water is 1 g/mL)** --- This guide serves as a comprehensive overview of the fundamental principles and calculations related to thermochemistry. It includes essential equations for calculating heat, enthalpy, entropy, and Gibbs free energy change, along with the associated constants. Practice problems are provided to test understanding and application of these concepts.
Transcribed Image Text: --- ### Unit 5 Study Guide #### Topics Covered: - Exothermic vs. Endothermic Reactions - Measuring Heat Flow (Specific Heat Capacity) - Enthalpy, Entropy, Gibbs Free Energy - Heats of Formation - Thermochemical Equations - Spontaneity of Reactions #### Equations: 1. **q = mCΔT** 2. **ΔH = ΣnΔH (products) - ΣnΔH (reactants)** 3. **ΔH_fusion = 334 J/g** 4. **ΔH_vaporization = 2260 J/g** 5. **q = mΔH_fusion** 6. **ΔG = ΣnΔG (products) - ΣnΔG (reactants)** 7. **q = mΔH_vaporization** 8. **ΔS = ΣnΔS (products) - ΣnΔS (reactants)** 9. **ΔG = ΔH - TΔS** #### Constants: - **C_water** = 4.184 J/g°C - **C_iron** = 0.449 J/g°C - **C_copper** = 0.385 J/g°C - **C_steam** = 2.03 J/g°C - **ΔH_fusion** = 334 J/g - **ΔH_vaporization** = 2260 J/g #### Practice Problems: 1. **A copper pot with a mass of 772 grams absorbs 2450 J of heat. Its final temperature is 137°C. What was its initial temperature?** 2. **How much heat is absorbed by a 15.5 g piece of gold as it is heated from 4.5°C to 177.4°C?** 3. **A container full of water absorbs 64.4 kJ of heat, and its temperature rises from 22.0°C to 73.4°C. What is the volume of water in mL? (The density of water is 1 g/mL)** --- This guide serves as a comprehensive overview of the fundamental principles and calculations related to thermochemistry. It includes essential equations for calculating heat, enthalpy, entropy, and Gibbs free energy change, along with the associated constants. Practice problems are provided to test understanding and application of these concepts.
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