its urgent pleaseIn the collision model it is assumed that reactions

occur as a result of collisions between molecules with

the correct kinetic energy and orientation. The

minimum energy required for a reaction to occur when

molecules collide is called the activation energy, $E_a.$

The number of collisions that are favorably oriented

for a reaction is described by the frequency factor, $A.$

The Arrhenius equation relates both of these factors

to the rate constant, $k$ :

$k=A*e^{-\frac{E_2}{R*T}}$

where $R=8\mathrm{.}314\frac{J}{\text{m}\text{o}\text{l}*K}$ and $T$ is the

temperature in kelvins.

$f=e^{-\frac{E_n}{R*T}}$

Most scientific calculators have an $e^x$ function as the second function of the $LN$ button.

Part B

A certain reaction with an activation energy of $205k\frac{J}{m}ol$ was run at $465K$ and again at $485K.$ What is the ratio of $f$ at the higher temperature to $f$ at the lower temperature?

Express your answer numerically using one significant figure.

View Available Hint$($s$)$

$\frac{f_{485}}{f_{465}}=$