Consider the following equilibrium at 800 K, C(s) + H_2O(g) CO(g) + H_2(g) Delta

Question

Consider the following equilibrium at 800 K, C(s) + H_2O(g) CO(g) + H_2(g) Delta H degree = +131 kJ K_c = 2.7 times 10^-2 I) Determine if the amount of CO(g) increases, decreases or remains unchanged under the following conditions: a) The temperature increases: b) The volume of the container decreases: II) Determine if the amount of H2(g) increases, decreases or remains unchanged under the following conditions: a) At 800 K, (H_2O) = 0.2M [CO] = 0.3M [H_2J = 0.5M with solid carbon present in the container. b) At 800 K, [H_2O] = [CO] and [H_2] = 0.01M with solid carbon present in the container.

Explanation / Answer

Hii,

(I) (a) as the reaction is endothermic and heat is given to the system the reaction will go forward therfore more CO will be produced

(b) as volume decreases reaction will go backward therfore CO will decrease

(II) in both the cases the reaction will go backward therfore H2 will decrease

Thank you

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