The rate constant of a reaction triples as the reaction temperature is raised by 10˚C from 25˚C to 35˚C.Calculate the activation energy for the reaction.

To solve this problem, we will use the Arrhenius equation which describes the temperature dependence of reaction rates. The equation is:

k = Ae^(-Ea/RT)

where: k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.

Given that the rate constant triples (k2/k1 = 3) when the temperature is raised by 10˚C (from 25˚C to 35˚C), we can set up the following equation using the Arrhenius equation:

k2/k1 = e^((Ea/R)(1/T1 - 1/T2))

where: k2 is the rate constant at T2, k1 is the rate constant at T1, T1 is the initial temperature in Kelvin, and T2 is the final temperature in Kelvin.

First, convert the temperatures from Celsius to Kelvin. T1 = 25˚C = 298.15 K and T2 = 35˚C = 308.15 K.

Substitute the given values into the equation:

3 = e^((Ea/R)(1/298.15 - 1/308.15))

Take the natural logarithm of both sides to solve for Ea/R:

ln(3) = (Ea/R)(1/298.15 - 1/308.15)

Rearrange the equation to solve for Ea:

Ea = R * ln(3) / (1/298.15 - 1/308.15)

The value of R (the gas constant) is 8.314 J/(mol*K) when Ea is in Joules. Substitute this value into the equation:

Ea = 8.314 J/(mol*K) * ln(3) / (1/298.15 - 1/308.15)

Calculate the value of Ea to find the activation energy for the reaction.