Two reactions R₁ and R₂ have identical pre-exponential factors. Activation energy of R₁ exceeds that of R₂ by 10 kJ mol^–1. If k₁ and k₂ are rate constants for reactions R₁ and R₂ respectively at 300 K, then ln(k₂/k₁) is equal to :
(R = 8.314 J mol^–1 K^–1)

The rate law for the reaction below is given by the expression k [A] [B]

A + B $$ \to $$ Product

If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below :

O₃(g) + Cl$${^ \bullet }$$ (g) $$ \to $$ O₂(g) + ClO$${^ \bullet }$$ (g) . . . . . .(i)

k_i = 5.2 × 10⁹ L mol⁻¹ s⁻¹

ClO$${^ \bullet }$$(g) + O$${^ \bullet }$$(g) $$ \to $$ O₂(g) + Cl$${^ \bullet }$$ (g) . . . . . . (ii)

k_ii = 2.6 × 10¹⁰ L mol⁻¹ s⁻¹

The closest rate constant for the overall reaction O₃(g) + O$${^ \bullet }$$ (g) $$ \to $$ 2 O₂(g) is :

Decomposition of H₂O₂ follows a first order reaction. In fifty minutes the concentration of H₂O₂ decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H₂O₂ reaches 0.05 M, the rate of formation of O₂ will be :