Q$1($AC: $2\mathrm{.}1$&$2\mathrm{.}2)$

Hydrogen peroxide reacts with iodide ions in acid conditions, as shown below.

$H_2{O}_2(aq)+2I^{-}(aq)+2H^{+}(aq)L_2(aq)+2H_{2}O(l)$

A student investigates the rate of this reaction by carrying out four experiments at the same

temperature. The student's results are shown below.

$($a$)$ The rate equation is: $,$ rate $=k[H_2{O}_2(aq)][r^{-}(aq)]$

Show that the student's results support this rate equation.

Calculate the rate constant, $k,$ for this reaction.

Give your answer to two significant figures, in standard form and with units.