6. Given the following methanation reaction at 1000 K. CO (g) + 3 H₂(g) → CH4 (g) + H₂O (g) AH = -230 kJ; Kc = 190 a. Is the conversion of the synthesis gas to methane favored at higher or lower temperature? Higher or lower pressure? b. What will be the mole fraction of CH4 (g) at equilibrium at 1000 K assuming you have 4.00 mol of synthesis gas with 1:3 mol ratio CO (g) to H₂ (g) in a 15.0 L reaction vessel.

6. Given the following methanation reaction at 1000 K. CO (g) + 3 H₂(g) → CH4 (g) + H₂O (g) AH = -230 kJ; Kc = 190 a. Is the conversion of the synthesis gas to methane favored at higher or lower temperature? Higher or lower pressure? b. What will be the mole fraction of CH4 (g) at equilibrium at 1000 K assuming you have 4.00 mol of synthesis gas with 1:3 mol ratio CO (g) to H₂ (g) in a 15.0 L reaction vessel.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 8RQ: Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What...

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Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
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