At equilibrium, the rate of the forward reaction is equal to therate of the reverse reaction. Both the forward and the reversereactions are occurring, but because they are occurring at the samerate, no change is observed in the appearance of the solution.

For this analysis, think about the affect that the addition orremoval of reactant will have on the rate of the forward reactionrelative to the rate of the reverse reaction at the instant thatthe reactant is added or removed. You also have to think about theaddition or removal of product on the rate of the reverse reactionrelative to the rate of the forward reaction.

a. When the concentration of reactant is increased for a systemat equilibrium, what is the effect on the rate of the forwardreaction? Does an increase in the rate of reactant have any effecton the rate of the reverse reaction? Explain your answer.

b. When the concentration of reactant is increased for a systemat equilibrium, which reaction is immediately faster – the forwardor the reverse reaction? Why?

c. As the reaction proceeds and the added reactant is used up,what happens to the rate of the forward reaction? At the point atequilibrium has been reached, what has happened to the rate of theforward reaction relative to the rate of the reverse reaction?

d. If reactant is removed from a system at equilibrium, what isthe effect on the rate of the forward reaction? Does the rate ofthe reverse reaction change when reactant is removed?

e. When reactant is removed in a system at equilibrium, whichreaction is faster – the forward reaction or the reverse reaction?Would that result in an accumulation of reactant or product in theflask?

f. Write a statement about why the addition of product causesthe reaction to shift to reactants in terms of the relative ratesof the forward and reverse reactions.

g. Write a statement from a kinetic perspective about why theremoval of reactant causes the reaction to shift towardsreactant.