Consider the following equilibrium: C(s) + H2O(g)  CO(g) + H2(g). (exothermic)

Question

List 2 factors that would cause the equilibrium to shift to the right(toward product)

List 2 factors that would cause the equilibrium to shift to the left (toward reactant)

Answer 1

According to Le Chatelier's principle, "a change in any of the components that determine a system's equilibrium conditions will move the equilibrium in such a way that the effect of the change is reduced or counteracted"

Factors that affect the equilibrium of a reaction include temperature, pressure, and concentration of reactants and products.

Factors that would cause the equilibrium to shift to the right (towards products)

1. increasing the concentration of one of more of the reactants (ex: increasing the concentration of C(s) or H2O(g) or increasing both)
2. decreasing the temperature. Since heat is a product of an exothermic reaction, decreasing the temperature is essentially decreasing the amount of product which would case a shift to the product to balance this out
3. decreasing the pressure. This causes a shift to the products because decreasing the pressure causes the number of moles of gas on the product side to decrease

Factors that would cause the equilibrium to shift to the left (towards reactants)

1. increasing the concentration of one of more of the products (ex: increasing the concentration of CO(g) or H2(g) or increasing both)
2. increasing the temperature. Since heat is a product of an exothermic reaction, increasing the temperature is essentially increasing the amount of product which would case a shift to the reactants to balance this out
3. increasing the pressure. This causes a shift to the reactants because increasing the pressure causes the number of moles of gas on the reactant side to decrease