Chemical Kinetics MCQs for NEET — Chemistry Questions with Answers

In gaseous reactions important for the understanding of the upper atmosphere H₂O and O react bimolecularly to form two OH radicals. $∆$H for this reaction is 72kJ at 500 K and E_a is 77 kJ mol^-1, then E_a for the bimolecular recombination of two OH radicals to form H₂O and O is:

For a reaction A$\stackrel{ }{\to }$ Product, rate law is $-\frac{d\left[A\right]}{dt}=K[A{]}_0$. The concentration of A left after time t when $t=\frac{1}{K}$ is:

For the reaction N₂ + 3H₂ $\to$ 2NH₃, the rate d[NH₃]/dt = 2x10^-4 Ms^-1 .Therefore, the rate -d[N₂]/dt is given as:

If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→  AB *, the rate of formation of AB * is directly proportional to:

In a reaction, the rate expression is, rate = K[A][B]^2/3[C]⁰ , the order of reaction is:

The rate of a reaction get doubles when the temperature changes from 7°C to 17°C. By what factor will it change for the temperature change from 17°C to 27°C?

For the elementary step,

(CH₃)_3.CBr(aq) → (CH₃)₃C⁺ (aq) + Br^- (aq) the molecularity is:

The rate of disappearance of SO₂ in the reaction; 2S0₂ +0₂ → 2S0₃ is 1.28 x10^-3g/sec. Then the rate of formation of SO₃ is:

When ethyl acetate was hydrolysed in pressure of 0.1 N HCl, the rate constant was found to be 5.40 x 10^-5 sec^-1 . But when 0.1 N H₂SO₄ was used for hydrolysis, the rate constant was found to be 6.25 X10^-5sec^-1. Thus, it may be concluded that:

The half time of a second order reaction is: