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$-1)$

$0\mathrm{.}1100\mathrm{.}0701\mathrm{.}83\backslash$times $10-1$

$0\mathrm{.}2200\mathrm{.}0353\mathrm{.}66\backslash$times $10-1$

$0\mathrm{.}2200\mathrm{.}0707\mathrm{.}32\backslash$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$).$

No

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

Yes

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

Yes

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

Yes

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

No

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

$1$ pts

Incorrect. Tries $3/5$ Previous Tries

For Rate $=-$d$[$ClO$2]/$dt$,$ calculate the rate constant $($k$).$

$($Units required.$)$

$1$ pts

Tries $0/5$

What would be the initial rate $(-$d$[$ClO$2]/$dt$)$ for an experiment with $[$ClO$2]0=0\mathrm{.}250$ mol$/$L and $[$OH$-]0=0\mathrm{.}0508$ mol$/$L$?$

$($Units required.$)$