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

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

$[$I$-]0[$OCl$-]0$ Initial Rate

$($mol$/$L$)($mol$/$L$)($mol L$-1$ s$-1)$

$0\mathrm{.}3600\mathrm{.}1008\mathrm{.}42\backslash$times $10-2$

$0\mathrm{.}0450\mathrm{.}1001\mathrm{.}05\backslash$times $10-2$

$0\mathrm{.}0900\mathrm{.}2004\mathrm{.}21\backslash$times $10-2$

$0\mathrm{.}1800\mathrm{.}2008\mathrm{.}42\backslash$times $10-2$

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

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

d$[$IO$-]/$dt $=$ k$[$OCl$-]3$

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

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

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

$1$ pts

Tries $0/5$

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

$($Units required.$)$