Question

Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift right, no change)

H2O(g) + C(s) ↔ H2(g) + CO(g) ∆H° = 131 kJ

a. increasing the temperature

b. adding CO

c. removing H2

c. removing H

e. increasing the volume of the container

f. adding more carbon to the reaction

Answer 1

(a) Here, enthalpy of the reaction is positive which means that heat is absorbed in the reaction. Then, on increasing temperature forward reaction is favored.

Therefore, shift right.

(b) On adding CO (adding product) backward reaction will be favored in order to attain the equilibrium again.

Therefore, shift left.

(c) On removing H2 (removing product) forward reaction will be favored in order to attain the equilibrium.

Therefore, shift right.

(e) On increasing volume of the container, reaction will occur such that there will be more gaseous products. Here, at the right more gaseous products than to the left.

Therefore, shift right.

(f) On adding C (adding reactant) forward reaction will be favored in order to attain the equilibrium.

Therefore, shift right.

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