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

For a reaction A + B → C + D if the concentration of A is doubled without altering the concentration of B, the rate gets doubled. If the concentration of B is increased by nine times without altering the concentration of A, the rate gets tripled. The order of the reaction is

In respect of the equation K = A–Ea / RT
e in chemical kinetics, which one of the following statements is correct?

The concentration of R in the reaction R → P was measured as a function of time and the following data is obtained

A reaction involving two different reactants can never be