Chemical Kinetics · Question 3

For an elementary chemical reaction, the Arrhenius plot is given below. [figure] If the energy of activation is 6.64 kJ mol-1 and R = 8.3 J K-1 mol-1, the temperature at which the rate constant becomes e2 min-1, is

1. 250 K
2. 125 K
3. 150 K
4. 200 K

2A k B is a zero-order reaction, where k = 1.0 mol L-1 min-1. If the initial concentration of A is 2 M, then the time taken to complete 75\% of the reaction will be

1. 2.0 min
2. 1.5 min
3. 0.75 min
4. 1.0 min

If the rate constant of a reaction is 0.03 s-1, how much time does it take for 7.2 mol L-1 concentration of the reactant to get reduced to 0.9 mol L-1 ? (Given: 2 = 0.301)

1. 210 s
2. 21.0 s
3. 69.3 s
4. 23.1 s

If the half-life (t1/2) for a first order reaction is 1 minute, then the time required for 99.9\% completion of the reaction is closest to :

1. 5 minutes
2. 10 minutes
3. 2 minutes
4. 4 minutes

Activation energy of any chemical reaction can be calculated if one knows the value of

1. rate constant at standard temperature
2. probability of collision
3. orientation of reactant molecules during collision
4. rate constant at two different temperatures

Which plot of k vs 1T is consistent with Arrhenius equation?

1. [figure]
2. [figure]
3. [figure]
4. [figure]

The rate of a reaction quadruples when temperature changes from 27 to 57 . Calculate the energy of activation. Given R = 8.314 J K-1 mol-1, 4 = 0.6021

1. 38.04 kJ/mol
2. 380.4 kJ/mol
3. 3.80 kJ/mol
4. 3804 kJ/mol

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

Which of the following plot represents the variation of k versus 1T in accordance with Arrhenius equation?

1. [figure]
2. [figure]
3. [figure]
4. [figure]

Rate constants of a reaction at 500 K and 700 K are 0.04 s-1 and 0.14 s-1, respectively; then, activation energy of the reaction is : (Given: 3.5 = 0.5441, R = 8.31 J K-1 mol-1)

1. 182310 J
2. 18500 J
3. 18219 J
4. 18030 J