When the temperature of a reaction increases from 27 oC to 37 oC, the rate increases by 2.5 times. The activation energy in the temperature range will be:
1. 53.6 kJ
2. 12.61 kJ
3. 7.08 kJ
4. 70.8 kJ
The graph that represents a first-order reaction is:
1. | 2. | ||
3. | 4. |
The rate of a reaction increases 4-fold when concentration of reactant is increased 16 times.
If the rate of reaction is 4 × 10-6 mol L-1s-1 when concentration of the reactant is 4 × 10-4 mol L-1, the rate constant of the reaction will be :
1. 2 × 10-4 m1/2 L-1/2 s-1
2. 1 × 10-2 s-1
3. 4 × 10-4 mol-1/2 L-1/2 s-1
4. 25 mol-1L min-1
If ‘a’ is the initial concentration of a substance which reacts according to zero-order kinetics and k is the rate constant, the time for the reaction to go to completion will be:
1. | a/k | 2. | 2/ka |
3. | k/a | 4. | Infinite |
The decomposition of a gaseous compound yields the following information:
Initial pressure, atm | 1.6 | 0.8 | 0.4 |
Time for 50 % reaction, min | 80 | 113 | 160 |
1. | 1.0 | 2. | 1.5 |
3. | 2.0 | 4. | 0.5 |
For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.
The order of the reaction will be:
1. 3
2. 2
3. 1
4. 0
The relationship between temperature and the variance in reaction rate is:
1. | 2. | ||
3. | 4. |
If a reaction A + B C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy of 70 kJ/mol, the activation energy for the reverse reaction will be:
1. 30 kJ/mol
2. 40kJ/mol
3. 70 kJ/mol
4. 100 kJ/mol
A first-order reaction takes 40 min for 30 % decomposition. The t1/2 for this reaction will be:
1. | 77.7 min | 2. | 27.2 min |
3. | 55.3 min | 4. | 67.3 min |
The half-life period for a first-order reaction is 20 minutes. The time required to change the concentration of the reactants from 0.08 M to 0.01 M will be:
1. | 20 minutes | 2. | 60 minutes |
3. | 40 minutes | 4. | 50 minutes |