The data below show the rate constant of a reaction measured at

several different temperatures.

Part A

Use an Arrhenius plot to determine the activation barrier for the reaction.

Express your answer in kilojoules per mole to three significant figures.

$E_a=65\mathrm{.}0k\frac{J}{m}ol$

Part B

Use an Arrhenius plot to determine frequency factor for the reaction.

Express your answer in reciprocal seconds to two significant figures.

$A=$

$s^{-1\text{P}\text{l}\text{e}\text{a}\text{s}\text{e}\text{h}\text{e}\text{l}\text{p}me\text{f}\text{i}\text{n}\text{d}\text{t}\text{h}\text{e}\text{a}\text{n}\text{s}\text{w}\text{e}\text{r}to\text{p}\text{a}\text{r}\text{t}B.}$