Consider the reaction:

N₂(g) + 3H₂(g) → 2NH₃(g)

The equality relationship between $\dfrac{\text{d}[NH_3]}{\text{d}t}$ and $\dfrac{\text{d}[H_2]}{\text{d}t}$ is

For the reaction: 2A + B → 3C + D, which of the following does not express the reaction rate?

The energies of activation for forward and reverse reactions for A₂ + B₂ ⇌ 2AB are 180 kJ mol^–1 and 200 kJ mol^–1 respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by 100 kJ mol^–1. The enthalpy change of the reaction (A₂ + B₂ → 2AB) in the presence of catalyst will be (in kJ mol^–1):

Rate of a reaction can be expressed by Arrhenius equation as: k = Ae^–E/RT In this equation, E represents

In a first order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is

For the reaction, N₂ + 3H₂ → 2NH₃, if $\dfrac{\text{d}NH_3}{\text{d}t}$ = 2 × 10^–4 mol L^–1 s^–1, the value of –$\dfrac{\text{d}H_2}{\text{d}t}$ would be

For a reaction $\dfrac{1}{2}$A → 2B, rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression:

For a first order reaction (A) → Product, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is:

Consider the reaction, 2A + B → Products. When concentration of B alone was doubled, the half–life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:

The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is