$3$ homework point$($s$)$

Rate Law from Initial Rates $($B$)$

$2$ClO$2($aq$)+2$OH$-($aq$)-->$ ClO$3-($aq$)+$ ClO$2-($aq$)+$ H$2$O$($l$)$

The above reaction was studied $($at a particular temperature$)$ and the following data $($for rate $=-$d$[$ClO$2]/$dt$)$ were obtained:

$[$ClO$2]0[$OH$-]0$ Initial Rate

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

$0\mathrm{.}1100\mathrm{.}1302\mathrm{.}55\backslash$times $10-1$

$0\mathrm{.}2200\mathrm{.}1301\mathrm{.}02$

$0\mathrm{.}2200\mathrm{.}0655\mathrm{.}10\backslash$times $10-1$

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

Note that the rate constant may be different for each of the choices below $($i$.$e$.$ k in choice A may be not equal to k in choice B etc$).$

Answers with YES OR NO

$1.-$d$[$ClO$2]/$dt $=$ k$[$ClO$2-]2[$OH$-]$

$2.-$d$[$ClO$2]/$dt $=$ k$[$OH$-][$ClO$2]$

$3.$ k$[$OH$-][$ClO$2]2=$ d$[$ClO$2-]/$dt

$4.$ d$[$ClO$3-]/$dt $=$ k$[$ClO$2][$OH$-]2$

$5.$ k$[$ClO$2]2[$OH$-]2=$ d$[$ClO$2-]/$dt