Chemical Kinetics

Match List-I with List-II :

1. A-IV, B-III, C-II, D-I
2. A-IV, B-III, C-I, D-II
3. A-I, B-II, C-III, D-IV
4. A-IV, B-II, C-I, D-III

Following data is for a reaction between reactants A and B : array|c|c|c| Rate ( mol L-1 s-1) & [A] & [B] \ 2 10-3 & 0.1 M & 0.1 M \ 4 10-3 & 0.2 M & 0.1 M \ 1.6 10-2 & 0.2 M & 0.2 M \ array The order of the reaction with respect to A and B, respectively, are

1. 1, 0
2. 0, 1
3. 1, 2
4. 2, 1

For a certain reaction, the rate = k[A]2[B], when the initial concentration of A is tripled keeping concentration of B constant, the initial rate would

1. increase by a factor of six
2. increase by a factor of nine
3. increase by a factor of three
4. decrease by a factor of nine

The decomposition of phosphine (PH3) on tungsten at low pressure is a first-order reaction. It is because the

1. rate is proportional to the surface coverage
2. rate is inversely proportional to the surface coverage
3. rate is independent of the surface coverage
4. rate of decomposition is very slow.

For a reaction between A and B the order with respect to A is 2 and the order with respect to B is 3. The concentrations of both A and B are doubled, the rate will increase by a factor of

1. 12
2. 16
3. 32
4. 10

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

1. rate = k[A][B]2
2. rate = k[A]2[B]2
3. rate = k[A][B]
4. rate = k[A]2[B]

The unit of rate constant for a zero order reaction is

1. mol L-1 s-1
2. L mol-1 s-1
3. L2 mol-2 s-1
4. s-1

Which one of the following statements for the order of a reaction is incorrect?

1. Order can be determined only experimentally.
2. Order is not influenced by stoichiometric coefficient of the reactants.
3. Order of a reaction is sum of power to the concentration terms of reactants to express the rate of reaction.
4. Order of reaction is always whole number.

During the kinetic study of the reaction, 2A + B C + D, following results were obtained array|l|l|l|l| Run & [A]/ mol L-1 & [B]/ mol L-1 & Initial rate of formation \ & & & of D/ mol L-1 min-1 \ I. & 0.1 & 0.1 & 6.0 10-3 \ II. & 0.3 & 0.2 & 7.2 10-2 \ III. & 0.3 & 0.4 & 2.88 10-1 \ IV. & 0.4 & 0.1 & 2.40 10-2 \ array Based on the above data which one of the following is correct?

1. Rate = k[A]2[B]
2. Rate = k[A][B]
3. Rate = k[A]2[B]2
4. Rate = k[A][B]2

For the reaction A + B products, it is observed that (i) on doubling the initial concentration of A only, the rate of reaction is also doubled and (ii) on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction. The rate of this reaction is given by

1. rate = k[A]2[B]2
2. rate = k[A][B]2
3. rate = k[A][B]
4. rate = k[A]2[B]

The bromination of acetone that occurs in acid solution is represented by this equation. CH3COCH3(aq) + Br2(aq) CH3COCH2Br(aq) + H+(aq) + Br-(aq) These kinetic data were obtained for given reaction concentrations. array|c|c|c|c| [CH3COCH3], M & [Br2], M & [H+], M & Initial rate, disappearance of Br2, M s-1 \ 0.30 & 0.05 & 0.05 & 5.7 10-5 \ 0.30 & 0.10 & 0.05 & 5.7 10-5 \ 0.30 & 0.10 & 0.10 & 1.2 10-4 \ 0.40 & 0.05 & 0.20 & 3.1 10-4 \ array Based on these data, the rate equation is

1. Rate = k[CH3COCH3][Br2][H+]2
2. Rate = k[CH3COCH3][Br2][H+]
3. Rate = k[CH3COCH3][H+]
4. Rate = k[CH3COCH3][Br2]

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 this reaction with respect to reactant B is

1. 2
2. -2
3. 1
4. -1

If the rate of the reaction is equal to the rate constant, the order of the reaction is

1. 0
2. 1
3. 2
4. 3

2A B + C It would be a zero order reaction when

1. the rate of reaction is proportional to square of concentration of A
2. the rate of reaction remains same at any concentration of A
3. the rate remains unchanged at any concentration of B and C
4. the rate of reaction doubles if concentration of B is increased to double

For the reaction; 2N2O5 4NO2 + O2 rate and rate constant are 1.02 10-4 and 3.4 10-5 s-1 respectively, then concentration of N2O5 at that time will be

1. 1.732
2. 3
3. 1.02 10-4
4. 3.4 105