Arrhenius Equation

A$($g$)+$ B$($g$)--->$ C$($g$)$

The rate law for the above reaction is:

$-$d$[$A$]/$dt $=$ k$[$A$][$B$]$

The rate constant is $3\mathrm{.}28\backslash$times $104$ L mol$-1$ s$-1$ at $304\mathrm{.}0\backslash$deg C and $2\mathrm{.}61\backslash$times $106$ L mol$-1$ s$-1$ at $497\mathrm{.}0\backslash$deg C$.$

Use the Arrhenius equation

k $=$ Ae$-$Ea$/$RT

to:

Calculate Ea for this reaction.

$8\mathrm{.}38\backslash$times $101$ kJ$/$mol

$1$ pts

You are correct.

Your receipt no$.$ is $162-4497$ Help: Receipt Previous Tries

A$.$Calculate the rate constant k at $379\mathrm{.}0\backslash$deg C for this reaction.

B$.$Calculate the pre$-$exponential factor A for this reaction.