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1. Consider the following equation: 2C2H2(g) + 502(g) → 4CO2(g) + 2H2O(g) + energy (a) Does the equation represent an endothermic reaction or an exothermic reaction? Justify your answer. (b) What effect would this reaction have on the temperature of its surroundings? Compare the temperature of the surroundings before the reaction takes place to the temperature of the surroundings after the reaction takes place. c) What does the equation communicate about the relative energy of the chemical bonds in the reactants and products? 2. Define and distinguish among the following terms: thermal energy, heat, and temperature. 3. Use the following information to answer the questions below: Q =m × c × AT %3D %3 heat (J) m=mass (g) c = specific heat capacity (J/g • °C) %3D AT = Tf- T; (°C) For water, c = 4.184 J/g • °C (a) A 50.0 g sample of water at 80.0 °C is mixed in a calorimeter with a 50.0 sample of water at 5.0 °C. What is the final temperature of the water?

1. Consider the following equation: 2C2H2(g) + 502(g) → 4CO2(g) + 2H2O(g) + energy (a) Does the equation represent an endothermic reaction or an exothermic reaction? Justify your answer. (b) What effect would this reaction have on the temperature of its surroundings? Compare the temperature of the surroundings before the reaction takes place to the temperature of the surroundings after the reaction takes place. c) What does the equation communicate about the relative energy of the chemical bonds in the reactants and products? 2. Define and distinguish among the following terms: thermal energy, heat, and temperature. 3. Use the following information to answer the questions below: Q =m × c × AT %3D %3 heat (J) m=mass (g) c = specific heat capacity (J/g • °C) %3D AT = Tf- T; (°C) For water, c = 4.184 J/g • °C (a) A 50.0 g sample of water at 80.0 °C is mixed in a calorimeter with a 50.0 sample of water at 5.0 °C. What is the final temperature of the water?

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Please the answer to question 1 ( a, b, and c) and question 2! Thank you! 

1. Consider the following equation: 2C2H2(g) + 502(g) → 4CO2(g) + 2H2O(g) + energy (a) Does the equation represent an endothermic reaction or an exothermic reaction? Justify your answer. (b) What effect would this reaction have on the temperature of its surroundings? Compare the temperature of the surroundings before the reaction takes place to the temperature of the surroundings after the reaction takes place. c) What does the equation communicate about the relative energy of the chemical bonds in the reactants and products?
Transcribed Image Text:1. Consider the following equation: 2C2H2(g) + 502(g) → 4CO2(g) + 2H2O(g) + energy (a) Does the equation represent an endothermic reaction or an exothermic reaction? Justify your answer. (b) What effect would this reaction have on the temperature of its surroundings? Compare the temperature of the surroundings before the reaction takes place to the temperature of the surroundings after the reaction takes place. c) What does the equation communicate about the relative energy of the chemical bonds in the reactants and products?
2. Define and distinguish among the following terms: thermal energy, heat, and temperature. 3. Use the following information to answer the questions below: Q =m × c × AT %3D %3 heat (J) m=mass (g) c = specific heat capacity (J/g • °C) %3D AT = Tf- T; (°C) For water, c = 4.184 J/g • °C (a) A 50.0 g sample of water at 80.0 °C is mixed in a calorimeter with a 50.0 sample of water at 5.0 °C. What is the final temperature of the water?
Transcribed Image Text:2. Define and distinguish among the following terms: thermal energy, heat, and temperature. 3. Use the following information to answer the questions below: Q =m × c × AT %3D %3 heat (J) m=mass (g) c = specific heat capacity (J/g • °C) %3D AT = Tf- T; (°C) For water, c = 4.184 J/g • °C (a) A 50.0 g sample of water at 80.0 °C is mixed in a calorimeter with a 50.0 sample of water at 5.0 °C. What is the final temperature of the water?
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