### Thermodynamics and Energy Changes**1. Calculate ΔE for each of the following. Indicate if the system does work on the surroundings or if the surroundings do work on the system.**a. $ q = -47 \, \text{kJ}, \, w = +88 \, \text{kJ} $b. $ q = +82 \, \text{kJ}, \, w = -47 \, \text{kJ} $c. $ q = +47 \, \text{kJ}, \, w = 0 \, \text{kJ} $---**2. A piston is compressed from a volume of 8.30 L to 2.80 L against a constant pressure of 1.90 atm. In the process, there is a heat gain by the system of 350 J. Calculate the internal energy change.**---**3. The equation for the fermentation of glucose to alcohol and carbon dioxide is:**\[ \text{C}_6\text{H}_{12}\text{O}_6 (\text{aq}) \rightarrow 2 \, \text{C}_2\text{H}_5\text{OH} (\text{aq}) + 2 \, \text{CO}_2 (\text{g}) \]**The enthalpy change for the reaction is -67 kJ. Is the reaction exothermic or endothermic?**Is energy, in the form of heat, absorbed or evolved as the reaction occurs?---This document covers the principles of thermochemistry, particularly focusing on the calculation of changes in internal energy ($\Delta E$) and the characteristics of reactions in terms of energy exchange. Make sure to apply the formula $ \Delta E = q + w $ for calculations and identify if a reaction is exothermic (releasing heat) or endothermic (absorbing heat) based on the given enthalpy change. **Thermodynamics Problems****4. Enthalpy of Combustion Problem:**The enthalpy of combustion of CH₄(g) when H₂O(l) is formed is -891 kJ/mol, and the enthalpy of combustion of CH₄(g) when H₂O(g) is formed is -803 kJ/mol. Use these data and Hess’s law to determine the enthalpy of vaporization of water.---**5. Combustion Reaction of Hydrocarbons:**When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₄H₄ (-2341 kJ/mol), C₄H₈ (-2755 kJ/mol), and H₂ (-286 kJ/mol), calculate ΔH for the reaction:\[ \text{C}_4\text{H}_4(g) + 2 \text{H}_2(g) \rightarrow \text{C}_4\text{H}_8(g) \]*Hint: Write the balanced equations for the combustion reactions of C₄H₄, C₄H₈, and H₂.*---**6. Chlorine Trifluoride Reaction:**Given the following data:1. $2 \text{ClF}(g) + \text{O}_2(g) \rightarrow \text{Cl}_2\text{O}(g) + \text{F}_2\text{O}(g)$ $ \quad ΔH = 167.4 \, \text{kJ} $2. $2 \text{ClF}_3(g) + 2 \text{O}_2(g) \rightarrow \text{Cl}_2\text{O}(g) + 3 \text{F}_2\text{O}(g)$ $ \quad ΔH = 341.4 \, \text{kJ} $3. $2 \text{F}_2(g) + \text{O}_2(g) \rightarrow 2 \text{F}_2\text{O}(g)$ $ \quad ΔH = -43.4 \, \text{kJ} $Calculate ΔH for the reaction:\[ \text{ClF}(g) + \text{F}_2(g) \rightarrow \text{

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Iculate föllowing. aicate if the system do work on the surroundings or the surroundings do work on the system. a. q=-47 kJ, w = +88 kJ b. q=+82 kJ, w = -47 kJ c. q=+47 kJ, w = 0 kJ

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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