CH4 (g) + H2O (g) CO (g) + 3H2 (g)

For this endothermic reaction, describe the direction the equilibrium position will shift towards as the pressure of the closed container is decreased by half?

A) The equilibrium position will shift to the right to produce more products.

B) The equilibrium position will shift to the left to produce more reactants.

C) The equilibrium position will shift in small increments to both the right and left.

D) The equilibrium position will not shift in response to the change in reaction conditions.

Question

Chemistry

Jacoby Hester

11 September, 17:04

CH4 (g) + H2O (g) CO (g) + 3H2 (g)

For this endothermic reaction, describe the direction the equilibrium position will shift towards as the pressure of the closed container is decreased by half?

A) The equilibrium position will shift to the right to produce more products.

B) The equilibrium position will shift to the left to produce more reactants.

C) The equilibrium position will shift in small increments to both the right and left.

D) The equilibrium position will not shift in response to the change in reaction conditions.

+4

Answers (1)

Know the Answer?

Brenton · Answer 1

Presuming the arrow is between H20 and CO

On the left there are 2 gas moles.

On the right there are 4 gas moles.

The equilibrium will shift to the side with the most no. He gas moles when pressure is decreased.

Therefore the answer is A, since 4>2.

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