Find the rate constant, given temperature and activation energy.

[Agent M27]

Homework Statement

A reaction is found to have an activation energy of 38.0 kJ/mol. If the rate constant for this reaction is 1.60 × 102 M-1s-1 at 249 K, what is the rate constant at 436 K?

Homework Equations

$$ln\frac{K_{2}}{K_{1}}=\frac{E_{a}}{R}\left(\frac{1}{T_{1}}-\frac{1}{T_{2}}\right)$$

The Attempt at a Solution

Given:

R=8.314
T₁=249K
T₂=436K
E_a=160

$$ln(K_{2})=\frac{38}{8.314}\left(\frac{1}{249}-\frac{1}{436}\right)+ln(160)$$

Which equals 161.257 which is incorrect. Any clues where I went wrong would be greatly appreciated. Thanks in advance.

Joe

 

[Borek]

38000

 

[Agent M27]

Ah ha! I should have noticed that being that R has units of J not Kj. Thank you very much Borek.

Joe

 

[Borek]

kJ, not Kj...