Indicate whether the statements are True or False. CHANGE any false ones to make them true! a) At equilibrium the amount of products must equal the amount of reactants. b) During equilibrium, the concentration of the products does not change. c) A collision between reactants is all that is needed to cause a reaction. d) At the beginning of a reaction the forward reaction is faster than the reverse reaction, but then the forward reaction slows down as the reverse reaction speeds up.

a. True

b. True

c. True

d. False

Explanation:

At equilibrium condition, the amount of products must be equal to the amount of reactants means 50% of reactant is converted into product and 50% of product is converted into reactant. During equilibrium, the concentration of the products as well as reactant does not change. Yes, a collision between reactants is needed to initiate and complete the reaction. If the concentrations of the reactants are too large, the rate of the forward reaction will be faster than the reverse reaction, and some of the reactants will be converted into products until equilibrium is achieved.

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