When the substances in the equation below are at
equilibrium at pressure P and temperature T, the
equilibrium can be shifted to favor the products by
MgO(s) + H₂(g) ⇆ Mg(s) + H₂O(g) ∆H = −14 kJ
a. increasing the pressure in the reaction vessel while
keeping the temperature constant
b. increasing the pressure by adding an inert gas such
as argon
c. decreasing the temperature
d. allowing some hydrogen gas to escape at constant
P and T
e. adding a catalyst