Question

The rate laws for the reaction:
$RCl+NaOH(aq.)\to ROH+NaCl$ is given by, $Rate=k_1\left[RCl\right].$ The rate of the reaction will be:

• A. Doubled on doubling the concentration of sodium hydroxide.
• B. Halved on reducing the concentration of alkyl halide to one half.
• C. Doubled on increasing the temperature of the reaction.
• D. Unaffected by increasing the temperature of the reaction.

Answer 1

The correct option is B Halved on reducing the concentration of alkyl halide to one half.

The rate law expression is $Rate=k_1\left[RCl\right].$

The rate of the reaction is independent of the concentration of NaOH. Hence, doubling the concentration of sodium hydroxide will not affect the rate of the reaction. Hence, option A is incorrect.

The reaction is of first order with respect to the concentration of alkyl halide. When the concentration of alkyl halide to one half, the rate of the reaction is also halved. Hence, the option B is true.

When the temperature of the reaction is increased, the rate of the reaction increases but it is not doubled. Hence, options C and D are incorrect.