Question

Q.2) For the reaction XY, the following data were obtained:

T/K 400 430

k/s-1 0.161 0.775

What is the value of activation energy?

Answer 1

To determine the activation energy for the reaction XY, we use the Arrhenius equation and the rate constants measured at two temperatures. After performing the calculations, we find that the activation energy is approximately 44.2 kJ/mol.

Step-by-step explanation:

Calculating Activation Energy

The question asks for the value of the activation energy for the reaction XY, based on the provided rate constants (k) at two different temperatures. To find the activation energy (Ea), we must use the Arrhenius equation, which is:

k = A * e(-Ea/(RT))

where:

Using the two-point form of the Arrhenius equation:

ln(k2/k1) = (Ea/R) * (1/T1 - 1/T2)

Plugging in the values:

ln(0.775/0.161) = (Ea/8.314) * (1/400 - 1/430)

After calculating the left-hand side and rearranging the equation to solve for Ea, we get:

Ea = ln(0.775/0.161) * 8.314 / (1/400 - 1/430)

By performing the calculations:

Ea = 0.41467 * 8.314 / (0.0025 - 0.002326)

Ea ≈ 44.2 kJ/mol

Therefore, the value of the activation energy for the reaction XY is approximately 44.2 kJ/mol.