10. Use data from your textbook’s appendix to determine ΔG° for the following reaction at 549 K and standard conditions:CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 193.7 kJ(b) ‒193.7 kJ(c) 5.749×104 kJ(d) ‒150.1 kJ11. Determine the equilibrium constant (K) for the reaction in the problem above. CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 481(b) 1.07×109(c) 2.08×10‒3(d) 1.87×1014 CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).H(kJ/mol) -108.6 0 -74.6 -241.8S (J.mol k) 218.8 130.7 186.3 188.8

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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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10. Use data from your textbook’s appendix to determine ΔG° for the following reaction at 549 K and standard conditions:
CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).
(a) 193.7 kJ

(b) ‒193.7 kJ

(d) ‒150.1 kJ

11. Determine the equilibrium constant (K) for the reaction in the problem above. CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).
(a) 481

(b) 1.07×109

(d) 1.87×1014

CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).

H(kJ/mol) -108.6 0 -74.6 -241.8

S (J.mol k) 218.8 130.7 186.3 188.8

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