You and your lab partner are studying the rate of a reaction, $A+B>C.$ You make measurements of the initial rate under the following conditions:

$\backslash$table$[[$Experiment $[A](M)[B](M),$Rate $(\frac{M}{s}),],[1,0\mathrm{.}3,0\mathrm{.}9],[2,0\mathrm{.}6,0\mathrm{.}9]]$

$)$

concentration of $C$ increases the rate by a factor of $3.$ Select the correct rate law for this reaction from the choices below.

Rate $=k[A][B][C]$

Rate $=k[A][C]$

Rate $=k[A{]}^2[C]$

Rate $=k[A][C{]}^2$

Rate $=k[A{]}^2[C{]}^2$

Rate $=k[A{]}^3[C]$

Rate $=k[A][C{]}^3$

$($c$)$ By what factor will the rate of the reaction described in part $($b$)$ above change if the concentrations of A$,$ B$,$ and C are all halved $($reduced by a factor of $2)?$

The rate will be the original rate multiplied by a factor of

$\backslash$table$[[$Experiment $[A](M)[B](M),$Rate $(\frac{M}{s}),],[1,0\mathrm{.}3,0\mathrm{.}9],[2,0\mathrm{.}6,0\mathrm{.}9]]$

$[$A

$[A]=0\mathrm{.}6$ and $[B]=0\mathrm{.}9$

$[A]=0\mathrm{.}3$ and $[B]=2\mathrm{.}7$

$[A]=0\mathrm{.}6$ and $[B]=1\mathrm{.}8$

$[A]=0\mathrm{.}6$ and $[B]=2\mathrm{.}7$

$[A]=0\mathrm{.}3$ and $[B]=1\mathrm{.}8$

$[A]=1\mathrm{.}2$ and $[B]=0\mathrm{.}9$

$[A]=0\mathrm{.}9$ and $[B]=0\mathrm{.}9$

$[A]=1\mathrm{.}5$ and $[B]=0\mathrm{.}9$ concentration of $C$ increases the rate by a factor of $3,$ Select the correct rate law for this reaction from the choices below.

Rate $=k[A][B][C]$

Rate $=k[A][C]$

Rate $=k[A{]}^2[C]$

Rate $=k[A][C{]}^2$

Rate $=k[A{]}^2[C{]}^2$

Rate $=k[A{]}^3[C]$

Rate $=k[A][C{]}^3$

$($c$)$ By what factor will the rate of the reaction described in part $($b$)$ above change if the concentrations of A$,$ B$,$ and C are all halved $($reduced by a factor of $2)?$

The rate will be the original rate multiplied by a factor of $\frac{1}{4}$