Agent M27
Sep18-10, 03:42 PM
1. The problem statement, all variables and given/known data
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?
2. Relevant equations
ln\frac{K_{2}}{K_{1}}=\frac{E_{a}}{R}\left(\frac{1 }{T_{1}}-\frac{1}{T_{2}}\right)
3. The attempt at a solution
Given:
R=8.314
T1=249K
T2=436K
Ea=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
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?
2. Relevant equations
ln\frac{K_{2}}{K_{1}}=\frac{E_{a}}{R}\left(\frac{1 }{T_{1}}-\frac{1}{T_{2}}\right)
3. The attempt at a solution
Given:
R=8.314
T1=249K
T2=436K
Ea=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