Question

Calculate the activation energy that leads to a doubling of the rate of reaction with an increase in temperature from 25∘c to 35∘c.

Answer 1

Take a look at the given formula fo activation energy, Ea. The R is the universal gas constant equal to 8.314 J/mol-K. Temperature is expressed in Kelvin. So,

T₁ = 25 + 273 = 298 K
T₂ = 35 + 273 = 308 K

Now, if you double the reaction, then that means K₂ = 2 K₁. So, the formula is reduced to

Ea = Rln(1/2)/(1/T₂ - 1/T₁)
Ea = 8.314 J/mol-K*ln(1/2)/(1/298 - 1/308)
Ea = -52,893.52 J