Chemical equilibrium

Chemical equilibrium occurs when the forward and reverse reactions proceed at:....

• a) A faster rate for the forward reaction than the reverse reaction

• b) Equal rates for both reactions

• c) A faster rate for the reverse reaction than the forward reaction

• d) Different rates for both reactions

When a reaction is at equilibrium, the concentrations of reactants and products:

• a) Continue to change constantly

• b) Stop changing and remain constant

• c) Increase without limit

• d) Decrease over time

At equilibrium, the rate of the forward reaction is:

• a) Greater than the rate of the reverse reaction

• b) Equal to the rate of the reverse reaction

• c) Less than the rate of the reverse reaction

• d) Zero

When a reaction reaches equilibrium, the reaction appears to stop because:

• a) The products are consumed faster than they are produced

• b) The forward reaction has a higher rate than the reverse reaction

• c) The concentrations of reactants and products remain constant

• d) The reverse reaction rate is much lower than the forward reaction rate

In a system at chemical equilibrium, the forward and reverse reactions occur at:

• a) Different rates, with the forward reaction being faster

• b) Equal rates, resulting in constant concentrations of reactants and products

• c) Only one rate, which is the rate of the forward reaction

• d) Zero rates after reaching equilibrium