In a reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, rate law for the reaction can be written as

Consider a reaction, aG + bH → Products. When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when the concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is:

The rate equation for the reaction: 2A + B → C is found to be: rate = k [A] [B]. The correct statement in relation to this reaction is that the

The velocity constant of a reaction at 290 K was found to be 3.2 × 10^–3 S^–1. When the temperature is raised to 310 K, it will be about:

The rate law for a reaction between the substances A an B is given by Rate = k [A]ⁿ[B]^m. On doubling the concentration of A and halving the concentration of B, the ratio of the new rate to the earlier rate of reaction will be

When a biochemical reaction is carried out in laboratory out side the human body in the absence of enzyme, then the rate of reaction obtained is 10^–6 times, than activation energy of reaction in the presence of enzyme is:

The rate equation for a reaction: A → B is r = K [A]°. If the initial concentration of the reactant is a mol dm^–3, the half life period of the reaction is

A follows first order reaction, A → product. Concentration of A, changes from 0.1 M to 0.025 M in 40 minutes. Find the rate of reaction of A when concentration of A is 0.01 M.

The rate of a first order reaction is 1.5 × 10^–2 mol L^–1 min^–1 at 0.5 M concentration of the reactant. The half life of the reaction is

Radioactivity of a sample (z = 22) decreases 90% after 10 years. What will be the half–life of the sample?