[Ready2Learn]

Hi all! I had a question....

Question 1: A reaction with activation energy of 123kJ/mole has  rate constant of 0.200s^-1 at 38 degrees Celsius. At what temperature will its rate constant be double that at 38 degrees Celsuis

Formula used: ln(k₂/k₁)=-(Ea/R)[(1/T₂)-(1/T₂)]

Attempt:  
T₁=(38+273K)=311K
T₂=?
Ea=123,000J/mole (needs to be converted from kJ->J)
R=8.314 J/mol*k
k₁=.200s^-1
k₂=(.200s^-1)(2)=.4s^-1

I was wondering how to change the formula for this particular question

I know you need to first get (1/T₂) and (1/T₁) on one side and -(Ea/R) and ln(k₂/k₁) on the other....would the ln(k₂/k₁) be divided by (Ea/R) or multiplied?

Thank you

[UG]

Say I let a =(1/T₂)-(1/T₁)
b = -(E_a/R)
and c = ln(k₁/k₂)
So that the equation becomes c = ba, how would you isolate 'a' on one side?