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(a) 2 NO(g) = N₂(g) + O₂(g) AH-[ If all gasses have partial pressures of 0.2 atm then AG - kJ/mol AS - J/mol-K AGⓇ = kJ/mol kJ/mol.

(a) 2 NO(g) = N₂(g) + O₂(g) AH-[ If all gasses have partial pressures of 0.2 atm then AG - kJ/mol AS - J/mol-K AGⓇ = kJ/mol kJ/mol.

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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Using values from Appendix C of your textbook, calculate the value of ΔH°, ΔS°, and ΔG° for each of the following reactions at standard temperature (298 K). Next, calculate ΔG if **all of the GASSES** in the reaction have partial pressures of **0.2 atm**. --- (a) \(2 \text{ NO(g)} \rightarrow \text{N}_2\text{(g)} + \text{O}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (b) \(\text{C}_6\text{H}_{12}\text{O}_6\text{(s)} \rightarrow 6 \text{ C(graphite)} + 6 \text{ H}_2\text{O(l)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (c) \(\text{CO(g)} + \text{H}_2\text{O(g)} \rightarrow \text{CO}_2\text{(g)} + \text{H}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (d) \(\text{N}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \rightarrow 2 \text{NO(g)} + 2 \text{H}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. ---
Transcribed Image Text:Using values from Appendix C of your textbook, calculate the value of ΔH°, ΔS°, and ΔG° for each of the following reactions at standard temperature (298 K). Next, calculate ΔG if **all of the GASSES** in the reaction have partial pressures of **0.2 atm**. --- (a) \(2 \text{ NO(g)} \rightarrow \text{N}_2\text{(g)} + \text{O}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (b) \(\text{C}_6\text{H}_{12}\text{O}_6\text{(s)} \rightarrow 6 \text{ C(graphite)} + 6 \text{ H}_2\text{O(l)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (c) \(\text{CO(g)} + \text{H}_2\text{O(g)} \rightarrow \text{CO}_2\text{(g)} + \text{H}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. --- (d) \(\text{N}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \rightarrow 2 \text{NO(g)} + 2 \text{H}_2\text{(g)}\) - ΔH° = ___ kJ/mol - ΔS° = ___ J/mol-K - ΔG° = ___ kJ/mol If all gasses have partial pressures of 0.2 atm then ΔG = ___ kJ/mol. ---
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