Using Le Châtelier's Principle

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Q1. Methanol, CH3OH, is finding use as a fuel additive. Describe the effect of each of the following changes on the equilibrium mixture for the following reaction:

2CH3OH(g) + 3O2(g) 2CO2(g) + 4H2O(g) + 1450 kJ

a. adding more CO2
b. adding more O2
c. increasing the volume of the container
d. increasing the temperature
e. adding a catalyst

Q2. Describe the effect of each of the following changes on the equilibrium mixture for the following reaction:

2HF(g) + Cl2(g) + 357 kJ 2HCl(g) + F2(g)

a. adding more Cl2
b. decreasing the volume of the container
c. increasing the temperature

a. When the concentration of the product CO2 increases, the equilibrium shifts in the direction of the reactants.
b. When the concentration of the reactant O2 increases, the equilibrium shifts in the direction of the products.
c. When the volume increases, the equilibrium shifts in the direction of the greater number of moles of gas, which is the products.
d. When the temperature is increased for an exothermic reaction, the equilibrium shifts in the direction of the reactants to remove heat.
e. When a catalyst is added, there is no change in the equilibrium mixture.

a. When the concentration of the reactant Cl2 increases, the equilibrium shifts in the direction of the products.
b. There is no change in equilibrium mixture because the moles of reactant are equal to the moles of product.
c. When the temperature for an endothermic reaction increases, the equilibrium shifts to remove heat, which is in the direction of the products.