The decomposition of AB given here in this balanced equation 2AB (g)⟶ A2 (g) + B2 (g), has rate constants of 8.58 x 10-9 L/mol s

Answer:

3.24 × 10^5 J/mol

Explanation:

To determine the activation energy for this reaction, the following equation is utilized:

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

Where; Ea is the activation energy (J/mol)

R represents the ideal gas constant = 8.3145 J/Kmol

T1 and T2 correspond to absolute temperatures (K)

k1 and k2 denote the reaction rate constants at the given temperatures

Initially, temperatures measured in °C must be converted to K

T(K) = T(°C) + 273.15

T1 = 325°C + 273.15

T1 = 598.15K

T2 = 407°C + 273.15

T2 = 680.15K

Given that k1= 8.58 x 10-9 L/mol, k2= 2.16 x 10-5 L/mol, and R= 8.3145 J/Kmol, we can now calculate Ea

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

ln(2.16 x 10-5/8.58 x 10-9) = Ea/8.3145 × (1/598.15 - 1/680.15)

ln(2517.4) = Ea/8.3145 × 2.01 × 10^-4

7.831 = Ea(2.417 × 10^-5)

Ea = 3.24 × 10^5 J/mol