Rate Law from Initial Rates

I$-($aq$)+$ OCl$-($aq$)->$ IO$-($aq$)+$ Cl$-($aq$)$

The above reaction was studied $($at a particular temperature$)$ and the following data were obtained:

$[$I$-]0($mol L$-1)[$OCl$-]0($mol L$-1)$ Initial Rate$($mol L$-1$ s$-1)$

$0\mathrm{.}1600\mathrm{.}1205\mathrm{.}64\backslash$times $10-2$

$0\mathrm{.}0400\mathrm{.}0607\mathrm{.}06\backslash$times $10-3$

$0\mathrm{.}3200\mathrm{.}0605\mathrm{.}64\backslash$times $10-2$

$0\mathrm{.}0800\mathrm{.}1202\mathrm{.}82\backslash$times $10-2$

Which of the following expressions for the rate law are completely consistent with the above experimental data.

$-$d$[$OCl$-]/$dt $=$ k$[$I$-][$OCl$-]2$

k$[$I$-][$OCl$-]=$ d$[$IO$-]/$dt

$-$d$[$I$-]/$dt $=$ k$[$OCl$-][$I$-]$

d$[$IO$-]/$dt $=$ k$[$I$-]2$

k$[$OCl$-]3=$ d$[$Cl$-]/$dt$1$

Calculate the rate constant $($k$).($Units required.$)$