A certain reaction has an activation energy of 52.50 kJ/mol. At what Kelvin temperature will the reaction proceed 7.50 times faster than it did at 295 K?

Question

please help

Answer 1

This problem uses a form of the Arrhenius equation:

ln k₂/k₁ = -Ea/R(1/T₂ - 1/T₁)

k₂ is the rate constant at temperature 2 (T2) = ?

k₁ is the rate constant at temperature 1 (T1) = 295

Ea is the activation energy = 52.50 kJ/mol 

k₂/k₁ = 7.50

R = 8.314 J/Kmol (note units of Ea; either change R or Ea to use same units)

Plug and chug and solve for T₂