Chemical Kinetics

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.

The rate constant of the reaction A B is 0.6 10-3 mol L-1 s-1. If the concentration of A is 5 M, then concentration of B after 20 minutes is

1. 3.60 M
2. 0.36 M
3. 0.72 M
4. 1.08 M

The activation energy of a reaction can be determined from the slope of which of the following graphs?

1. k vs. 1T
2. T k vs. 1T
3. k vs. T
4. kT vs. T

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is

1. second
2. more than zero but less than first
3. zero
4. first.

A reaction having equal energies of activation for forward and reverse reactions has

1. H = 0
2. H = G = S = 0
3. S = 0
4. G = 0

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20 C to 35 C? (R = 8.314 J mol-1 K-1)

1. 34.7 kJ mol-1
2. 15.1 kJ mol-1
3. 342 kJ mol-1
4. 269 kJ mol-1

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

A reaction is 50\% complete in 2 hours and 75\% complete in 4 hours. The order of reaction is

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

Activation energy (Ea) and rate constants (k1 and k2) of a chemical reaction at two different temperatures (T1 and T2) are related by

1. k2k1 = - EaR ( 1T1 - 1T2 )
2. k2k1 = - EaR ( 1T2 - 1T1 )
3. k2k1 = - EaR ( 1T2 + 1T1 )
4. k2k1 = EaR ( 1T1 - 1T2 )

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]