Question

For the reaction of a and b forming c, a(aq) + b(s) ⇌ 2c(aq), how will the reaction respond to each of the following changes at equiLiBrium?

1) Increase the concentration of a
2) Decrease the concentration of b
3) Increase the temperature
4) Add a catalyst

Answer 1

Increasing the concentration of a reactant will favor the forward reaction. Decreasing the concentration of a reactant will favor the reverse reaction. Increasing the temperature favors the endothermic reaction. Adding a catalyst does not affect the position of the equilibrium.

Step-by-step explanation:

When the concentration of reactant a is increased at equilibrium, the reaction will shift to the right (forward reaction) to consume the excess a and form more of product c. This is because according to Le Chatelier's principle, increasing the concentration of a reactant will favor the forward reaction to decrease the excess concentration.

When the concentration of reactant b is decreased at equilibrium, the reaction will shift to the left (reverse reaction) to replenish the decreased concentration of b. This is because decreasing the concentration of a reactant will favor the reverse reaction to increase the concentration of b.

When the temperature is increased at equilibrium, the reaction will shift in the endothermic direction, which is the forward reaction in this case. This is because increasing the temperature favors the endothermic reaction, which absorbs heat from the surroundings.

Adding a catalyst does not affect the position of the equilibrium. It increases the rate of both the forward and reverse reactions equally, allowing the system to reach equilibrium faster but without any change in the equilibrium concentrations of reactants and products.