When the concentration of reactant is increased for a system at equilibrium, wha
ID: 998065 • Letter: W
Question
When the concentration of reactant is increased for a system at equilibrium, what is the effect on the rate of the forward reaction? Does an increase in the rate of reactant have any effect on the rate of the reverse reaction? Explain your answer. When the concentration of reactant is increased for a system at equilibrium, which reaction is immediately faster - the forward or the reverse reaction? Why? As the reaction proceeds and the added reactant is used up, what happens to the rate of the forward reaction? At the point at equilibrium has been reached, what has happened to the rate of the forward reaction relative to the rate of the reverse reaction? If reactant is removed from a system at equilibrium, what is the effect on the rate of the forward reaction? Does the rate of the reverse reaction change when reactant is removed? When reactant is removed in a system at equilibrium, which reaction is faster - the forward reaction or the reverse reaction? Would that result in an accumulation of reactant or product in the flask? Write a statement about why the addition of product causes the reaction to shift to reactants in terms of the relative rates of the forward and reverse reactions. Write a statement from a kinetic perspective about why the removal of reactant causes the reaction to shift towards reactant.Explanation / Answer
Le Châtelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium. If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change.
(a) When the concentration of reactant is increased at equilibrium, the rate of forward reaction increases. Applying Le Chatelier's Principle,an increase in concentration on one side of an equation favors or drives the reaction to the opposite side. Adding reactants favors products, and adding products favors reactants.
It does not have any effect on reverse reaction.
(b) When the concentration of reactant is increased at equilibrium, forward reaction is immediately faster.
Le Châtelier's principle states that if the system is changed in a way that increases the concentration of one of the reacting species, it must favor the reaction in which that species is consumed.
(c) As the reaction proceeds and the added reactant is used up, the rate of forward reaction decreases.
At the point equilibrium has been reached, rate of forward reaction becomes equal to the rate of backward reaction.
(d) If a reactant is removed from a system at equilibrium, the rate of forward reaction decreases and the rate of backward reaction increases.
(e) When the reactant is removed at equilibrium, backward reaction is faster. It will result in the accumulation of reactant in the flask.
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