Pre$-$Equilibria Conditions in Reaction Mechanisms

CO$($g$)+$ Cl$2($g$)-->$ COCl$2($g$)$

The above reaction obeys the mechanism:

Cl$2=2$Cl Fast equilibrium

Cl $+$ CO $=$ COCl Fast equilibrium

COCl $+$ Cl$2-->$ COCl$2+$ Cl Slow

$2$Cl $-->$ Cl$2$ Fast

Consider each of the following expressions and select "Yes" or $"$No$"$ to indicate which represent a correct statement of the rate law that is consistent with the given mechanism.

Yes or No for the answers

$1.$d$[$COCl$2]/$dt $=$ k$[$Cl$]2$

$2.-$d$[$Cl$2]/$dt $=$ k$[$Cl$2]3/2[$CO$]$

$3.$ d$[$COCl$2]/$dt $=$ k$[$CO$][$Cl$2]3/2$

$4.$ d$[$COCl$2]/$dt $=$ k$[$CO$][$Cl$]$

$5.$ d$[$COCl$2]/$dt $=$ k$[$Cl$2]2[$CO$]$

$6.-$d$[$CO$]/$dt $=$ k$[$Cl$2]3/2[$CO$]$

$1$ pts

Tries $0/15$

Suppose that: k$1/$k$-1=1\backslash$times $10-2$ mol L$-1,$ k$2/$k$-2=1\backslash$times $106$ L mol$-1,$ k$3=1\backslash$times $10-4$ L mol$-1$ s$-1,$ and k$4=1\backslash$times $103$ L mol$-1$ s$-1.$

B$.$What would be the value of the overall rate constant, k$,$ including the correct units?