Question

n the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right?

CO(g) + 3H2 (g)CH4 (g) + H2O (g) H = -206 kJ/mol

decreasing the concentration of carbon monoxide (CO)

increasing the volume of the reaction system

decreasing the concentration of hydrogen gas (H2)

lowering the temperature of the reaction

Answer 1

This is a LeChatlier's Principle question.

Decreasing concentration of any compound forces the equilibrium to shift to that side.
Increasing the volume of the reaction forces the equilibrium to shift to the side with a greater coefficient sum.
Lowering the temperature of the reaction (negative enthalphy means exothermic) forces the equilibrium to the products.

Does that help?