The temperature dependence of the rate constant (k) of a chemical reaction is written in terms of the Arrhenius equation,
k = A.e–E*/RT. The activation energy (E*) of the reaction can be calculated by plotting:
1.
2.
3.
4.
The radioisotope, tritium has a half-life of 12.3 years. If the initial amount of tritium is 32 mg, how many milligrams of it would remain after 49.2 years:
1. | 1 mg | 2. | 2 mg |
3. | 4 mg | 4. | 8 mg |
The half-life period of is:
1. 500 years
2. 5000 years
3. 50 years
4. 5 × years
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 |
The reaction A → B follows first-order kinetics. The time taken for 0.8 mol of A to produce 0.6 mol of B is 1 hour. The time taken for the conversion of 0.9 mol of A to produce 0.675 mol of B will be:
1. | 1 hour | 2. | 0.5 hour |
3. | 0.25 hour | 4. | 2 hour |
The activation energy for a simple chemical reaction A → B is Ea in a forward direction. The activation energy for the reverse reaction:
1. Is negative of Ea
2. Is always less than Ea
3. Can be less than or more than Ea
4. Is always double of Ea
When a biochemical reaction is carried out in a laboratory outside the human body in the absence of an enzyme, then the rate of reaction obtained is times. The activation energy of a reaction in the presence of an enzyme is:
1.
2. P is required.
3. Different from obtained in the laboratory.
4. Data is insufficient.
If at a given instant, for the reaction 2N2O5 → 4NO2 + O2 rate and rate constant are 1.02 × 10-4 and 3.4 × 10-5 sec -1 respectively, then the concentration of at that time will be:
1. 1.732
2. 3.0
3.
4.
; It would be a zero-order reaction when:
1. | The rate of reaction is proportional to the square of the concentration of A |
2. | The rate of reaction remains the 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 the concentration of B is doubled |
rate of reaction is equal to:-
1.
2.
3.
4.