Test: Chemical Kinetics - 3 - Chemistry MCQ

Rate of a reaction. A + B → Product is given below as a function of different initial concentrations of A and B.

The rate of the reaction is:

In a reaction: 2N₂O₅ → 4NO₂ + O₂ , the rate is expressed as

The relation among K₁, K₂ and K₃ is:

Calculate order of reaction A → product , from the following data:

A first order reaction is 50% complete in 30mins at 27⁰C and in 10mins at 47⁰C. At 27⁰C, the activation energy of the reaction in KJ/mole is:

What is the rate of simple reaction 2NO + O₂ → 2 NO₂ ; when the volume of the reaction vessel is doubled?

Which among the following procedures will lead to a change in rate constant ‘k’ of a reaction?

(I) A change in pressure
(II) Change in temperature
(III) Change in volume of the reaction vessel
(IV) An introduction of a catalyst

The concept of t_1/2 is useful for the reaction of:

For a given set of reactions:

The rate constant for the decay of N₂O₅ depends on:

The given reaction (pre-equilibrium mechanism)

The gas phase decomposition of NOBr is second order in [NOBr], with k = 0.810 M^–1 s^–1 at 10⁰C. We start with in a flask at 10⁰C. How many seconds does it take to use up

2NOBr(g) → 2NO(g) + Br₂(g)

Rate = k[NOBr]²

The concentration of a reactant undergoing decomposition was 0.1, 0.08 and 0.067 mol L^–1 after 1.0, 2.0 and 3.0 hr respectively. The order of the reaction is:

Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is:

A reaction of first-order completed 90% in 90 minutes, hence, it is completed 50% in approximately.

The unit of catalytic constant is equal to:

At 350K, the effective rate constant for a gaseous reaction A → P , which has a Lindeman-Hinshelwood mechanism are and  respect ively. The rate constant for activation step in the mechanism is:

In the temperature range of 250 K to 450 K, the pre-exponent ial factor, A, for the reaction. Cl(g) + H₂(g) → HCL(g) + H(g) is found to be equal to 1.20 x 10¹⁰ dm³ mol^-1 s^-1 . If M (Cl) = 35.453 g mol^-1, M[H₂] = 2.016 g mol^-1, d(Cl) = 200 pm and d[H₂] = 150 pm, the value of the Steric factor, P is:

The t_1/2 of a reaction is doubled as the initial concentration of a reactant is increased 4 times. The order of the reaction is:

The relaxation time for the fast reaction:

and equilibrium constant is 1.0 x 10^–3. The rate constant of the backward reaction is:

For which of the following reactions, the rate constant will be independent of ionic strength.

(I) H⁺ + Br^– + H₂O₂
(II) C₂H₅COOCH₃ + OH^–
(III) S₂O₃^2– + I^–

Which of the following plots is correct for an ionic reaction:

For the first order isomerization of an organic compound at 130⁰C, the activation energy is 108.4 KJ mol^–1 and the rate constant is 9.12 x 10^–4 s^–1. The standard entropy of activation for this reaction is:

For reaction system,

2NO(g) + O₂ (g) → 2 NO₂ (g)

Volume is suddenly reduced to half of its value by increasing the pressure on it. If the reaction is of first order with respect to O₂ and second order with respect to NO, the rate of reaction will.

Rate = K[A][B]; If the volume of reaction vessel is suddenly reduced 1/4^th of initial value. The new rate will be effected by:

Under the same reaction conditions, initial concentration of 1.386 mol dm^–3 of a substance becomes half in 40 s and 20 s through first order and zero order kinetics, respectively., Ratio  of the rate constants for the first order k₁ and zero order (k₀) of the reaction is 

T₅₀ (Half-life period) of first-order reaction is 10 minute. Starting with 10 mol L^–1. Rate after 20 minute is:

If the fermentation of sugar in an enzymatic solution that in 0.12 M. the concentration of the sugar is reduced to 0.06 M in 10 h and to 0.03 M in 20 h. What is the order of the reaction:

In a zero-order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become