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Consider the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 208K, the data available are: ∆fH°CH4 = -74.85 kJ/ mol ∆fS°CH4 = -80.67 J/ mol K ∆fG°c,graphite = ∆fG° H2(g)=0 a. Calculate the equilibrium constant (K) of the dissociation of methane at 298 K with the appropriate units. b. Assuming that ∆H is independent of temperature, calculate the equilibrium constant (K) of methane dissociation at 1000 K c. Calculate the ratio between the amounts of methane and hydrogen gases at 298 K and 0.2 barg

Consider the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 208K, the data available are: ∆fH°CH4 = -74.85 kJ/ mol ∆fS°CH4 = -80.67 J/ mol K ∆fG°c,graphite = ∆fG° H2(g)=0 a. Calculate the equilibrium constant (K) of the dissociation of methane at 298 K with the appropriate units. b. Assuming that ∆H is independent of temperature, calculate the equilibrium constant (K) of methane dissociation at 1000 K c. Calculate the ratio between the amounts of methane and hydrogen gases at 298 K and 0.2 barg

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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Consider the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 208K, the data available are: ∆fH°CH4 = -74.85 kJ/ mol ∆fS°CH4 = -80.67 J/ mol K ∆fG°c,graphite = ∆fG° H2(g)=0 a. Calculate the equilibrium constant (K) of the dissociation of methane at 298 K with the appropriate units. b. Assuming that ∆H is independent of temperature, calculate the equilibrium constant (K) of methane dissociation at 1000 K c. Calculate the ratio between the amounts of methane and hydrogen gases at 298 K and 0.2 barg.
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