# A-level Chemistry/OCR (Salters)/Kinetics

## Rate equations

${\displaystyle {\mbox{rate}}=k[A]^{m}[B]^{n}\,\!}$

${\displaystyle {\mbox{order of reaction}}=m+n\,\!}$

## Arrhenius equation

${\displaystyle k=Ae^{-{\frac {E_{a}}{RT}}}}$

### Arrhenius plot

${\displaystyle \ln {(k)}=\ln {\left(Ae^{-{\frac {E_{a}}{RT}}}\right)}}$

${\displaystyle \ln {(k)}=\ln {(A)}+\ln {\left(e^{-{\frac {E_{a}}{RT}}}\right)}}$

${\displaystyle \ln {(k)}=\ln {(A)}+-{\frac {E_{a}}{RT}}}$

${\displaystyle \ln {(k)}=\ln {(A)}-{\frac {E_{a}}{RT}}}$

${\displaystyle \ln {(k)}=-{\frac {E_{a}}{RT}}+\ln {(A)}}$

${\displaystyle \ln {(k)}=-{\frac {E_{a}}{R}}{\frac {1}{T}}+\ln {(A)}}$

${\displaystyle {\mbox{straight-line graphs are always of the form }}y=mx+c\,\!}$

${\displaystyle {\mbox{therefore, the dependent variable }}y{\mbox{ is }}\ln {(k)}\,\!}$

${\displaystyle {\mbox{the gradient }}m{\mbox{ is }}-{\frac {E_{a}}{R}}\,\!}$

${\displaystyle {\mbox{the independent variable }}x{\mbox{ is }}{\frac {1}{T}}\,\!}$

${\displaystyle {\mbox{the y-intercept }}c{\mbox{ is }}\ln {(A)}\,\!}$