(Q91) The activation energy for a certain reaction is -179 kJ/mol. If the rate constant is 116 M-1s1 at 11.2 °C, what will the numerical value of the rate constant be at 23.2 °C?

Calculate the rate constant, k, for a reaction at 57.0 °℃ that has an activation energy of 83.5 kJ/mol and a frequency factor -1 of 8.97 x 10¹1 s k = 8-1

Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) à H2O(g) + N(g) Ea = 436 kJ ∆H = –491 kJ (ii) N(g) + NO(g) à N2(g) + O(g) Ea = 625 kJ ∆H = –312 kJ (iii) O(g) + H2(g) à H2O(g) Ea = 1690 kJ ∆H = +131 kJ Draw the potential energy diagram for the reaction. Assume the potential energy of the reactants was 1400 kJ

A reversible reaction that occurs in a single step has AH= -26.2 kJ/mol and Ea = 25.2 kJ/mol. What is the activation energy of the reverse reaction? kJ/mol