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Problem 13.30.

Following are two statements pertaining to the reaction 2A + B
2C, for which the rate law is *rate* = *k*[A][B]. Identify which
statement is true and which is false, and explain your reasoning.

(**a**) The value of *k* is *independent* of the initial
concentrations [A]_{0} and [B]_{0}.

(**b**) The unit of the rate constant for this reaction can be expressed
either as s^{–1} or min^{–1}.

The rate law is second order overall. The rate constant, by definition,
is independent of concentrations, initial or otherwise, so (**a**) must
be true. The units of the rate constant for a second order reaction are
M^{–1}s^{–1} or M^{–1}min^{–1} (rate =
Ms^{–1} = k[M][M]) so (**b**) is false.