The reaction between ethyl bromide $($C$2$H$5$Br$)$

and hydroxide ion in ethyl alcohol at $330$ K

is first order each in ethyl bromide and the hydroxide ion:

C$2$H$5$Br$($alc$)+$OH$($alc$)->$C$2$H$5$OH$($l$)+$Br$($alc$)$

When $[$C$2$H$5$Br$]$

is $0\mathrm{.}0447$ M

and $[$OH$]$

is $0\mathrm{.}100$ M

$,$ the rate of disappearance of ethyl bromide is $1\mathrm{.}7\backslash$times $107$

M$/$s

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