Review I Constants I Periodic Table

The reaction between ethyl bromide $(C_2{H}_{5}Br)$ and hydroxide ion in ethyl alcohol at $330K$ is first order each in ethyl bromide and the hydroxide ion:

$C_2{H}_{5}Br($ alc $)+O{H}^{-}(alc)C_2{H}_{5}OH(l)+B{r}^{-}(alc)$

When $C_2{H}_{5}Br$ is $0\mathrm{.}0427M$ and $O{H}^{-}$is $0\mathrm{.}110M,$ the rate of disappearance of ethyl bromide is $1\mathrm{.}5{10}^{-7}\frac{M}{s}.$

Part A

Part B

Part C

How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding two equal volumes of pure ethyl alcohol to the solution?

The rate would be

devided by $3$

multiplied by $3$

the same

multiplied by $\frac{1}{9}$

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