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:

(1) H₂SO₄ is stronger than HCI

(2) H₂SO₄ is weaker than HCl

(3) H₂SO₄ and HCl both have the same strength

(4) the data are not sufficient to compare the strength of H₂SO₄ and HCI

The half time of a second order reaction is:

(1) inversely proportional to the square of the initial concentration of the reactants

(2) inversely proportional to the initial concentration of the reactants

(3) proportional to the initial concentration of reactants

(4) independent of the initial concentration of reactants

The half-life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301):

(a) 23.03 minutes

(b) 46.06 minutes

(c) 460.6 minutes

(d) 230.3 minutes

A zero order reaction is one:

(1) In which reactants do not react

(2) In which one of the reactants is in large excess

(3) Whose rate does not change with time

(4) Whose rate increases with time

For A+B $\to$C+D, $∆$H = -20 kJmol^-1 the activation energy of the forward reaction is 85 kJ mol^-1. The activation energy for backward reaction is...... kJ mol^-1

1. 105

2. 85

3. 40

4. 65

For the elementary reaction M $\to$ N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M is:

(1) 4

(2) 3

(3) 2

(4) 1

The rate constant for a second order reaction is 8x10^-5 M^-1 min^-1 . How long will it take a 1M solution to be reduced to 0.5M?

(1) 8.665 x 10³ minute

(2) 8 x 10^-5 minute

(3) 1.25 x 10⁴ minute

(4) 4x10^-5 minute

The time for the half-life of a first-order reaction is 1 hr. The time taken for 87.5% completion of the reaction is-

1. 1 hour

2. 2 hour

3. 3 hour

4. 4 hour

Which order of reaction obeys the relation t_1/2 = 1/Ka?

(a) First

(b) Second

(c) Third

(d) Zero

The chemical reaction, 2O₃ $\to$3O₂ proceeds as follows;

O₃ $\rightleftharpoons$O₂ + O .....(Fast)

O+O₃ $\to$ 2O₂ ....(Slow)

The rate law expression should be:

(a) r = K[O₃]²

(b) r = K[O₃]²[O₂]^-1

(c) r = K[O₃][O₂]

(d) unpredictable