For a reaction taking place in four different steps, the rate constants follow a relationship $K-\frac{K_2K_4}{K_1K_3}$ . If the energies of activation E 1 , E 2 , E 3 and E 4 are 10 kJ/mol, 30kJ/mol, 40 kJ/mol and 20 kJ/mol respectively, then the overall energy of activation would be :

Question

cdquestions Admin · Accepted Answer

The correct option is (A) :Zero kJ/mol.

Answer

Zero kJ/mol

Answer

Answer

Answer

1000 kJ/mol

For a reaction taking place in four different steps, the rate constants follow a relationship \(K-\frac{K_2K_4}{K_1K_3}\). If the energies of activation E₁, E₂, E₃ and E₄ are 10 kJ/mol, 30kJ/mol, 40 kJ/mol and 20 kJ/mol respectively, then the overall energy of activation would be :

The Correct Option is A

Solution and Explanation

Top Questions on Gibbs energy change and equilibrium

Questions Asked in CUET exam

For a reaction taking place in four different steps, the rate constants follow a relationship \(K-\frac{K_2K_4}{K_1K_3}\). If the energies of activation E1, E2, E3 and E4 are 10 kJ/mol, 30kJ/mol, 40 kJ/mol and 20 kJ/mol respectively, then the overall energy of activation would be :

The Correct Option is A

Solution and Explanation

Top Questions on Gibbs energy change and equilibrium

Questions Asked in CUET exam

For a reaction taking place in four different steps, the rate constants follow a relationship \(K-\frac{K_2K_4}{K_1K_3}\). If the energies of activation E₁, E₂, E₃ and E₄ are 10 kJ/mol, 30kJ/mol, 40 kJ/mol and 20 kJ/mol respectively, then the overall energy of activation would be :