Consider the following data concerning the equation:

$]$

$1$

$[H^{+}$

II$.,0\mathrm{.}100M,1\mathrm{.}00{10}^{-3}M,1\mathrm{.}00{10}^{-2}M,0\mathrm{.}268\frac{M}{sec}$

III. $0\mathrm{.}200M,1\mathrm{.}00{10}^{-3}M1\mathrm{.}00{10}^{-2}M0\mathrm{.}542\frac{M}{sec}$

IV$.,0\mathrm{.}400M,1\mathrm{.}00{10}^{-3}M2\mathrm{.}00{10}^{-2}M1\mathrm{.}084\frac{M}{sec}$

The rate law for this reaction is

a$.$ rate $=k[H_2{O}_2][I^{-}]$

b$.$ rate $=k[H_2{O}_2{]}^2[I^{-}{]}^2[H^{+}{]}^2$

c$.$ rate $=k[I^{-}][H^{+}]$

d$.$

rate $=k[H_2{O}_2][I^{-}][H^{+}]$

e$.$ rate $=k[H_2{O}_2][H^{+}]$