1. For each of the following rate equations, describe what would happen to the rate if the concentration of reactant A was tripled and the concentration of reactant B is halved.

a. Rate = k[A][B]

b. Rate = k[A]2 [B]

c. Rate = k[A]2 [B]2

d. Rate = k[A][B]

2. If a reactant is used up according to a first order rate equation, and the initial concentration of the reactant is 3.2 mol L-1 , what is the concentration of the reactant after two half-lives have passed, and after six half-lives have passed?

Question

1. For each of the following rate equations, describe what would happen to the rate if the concentration of reactant A was tripled and the concentration of reactant B is halved.

a. Rate = k[A][B]

b. Rate = k[A]2 [B]

c. Rate = k[A]2 [B]2

d. Rate = k[A][B]

2. If a reactant is used up according to a first order rate equation, and the initial concentration of the reactant is 3.2 mol L-1 , what is the concentration of the reactant after two half-lives have passed, and after six half-lives have passed?

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