The rate law of the reaction,
$\mathrm{RCl}+\mathrm{NaOH}\to \mathrm{ROH}+\mathrm{NaCl}$ is given by
Rate $=\mathrm{k}\left[\mathrm{RCl}\right]$. The rate of this reaction
A) is doubled by doubling the concentration of $\mathrm{NaOH}$

B) is halved by reducing the concentration of $\mathrm{RCl}$ to half

C) is increased by increasing the temperature of the reaction

D) is unaffected by change in temperature
Which is correct?