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Q. No.The decomposition of N2O5 in CCl4 at 318K has been studied by monitoring the concentration of N2O5 in the solution. Initially, the concentration of N2O5 is 2.33 mol L–1 and after 184 minutes, it is reduced to 2.08 mol L–1. The reaction takes place according to the equation
2 N2O5 (g) → 4 NO2 (g) + O2 (g)
The rate of production of NO2 during this period is-
1. 5.72 × 10–3 mol L–1 min–1
2. 2.72 × 10–3 mol L–1 min–1
3. 1.72 × 10–5 mol L–1 min–1
4. 6.72 × 10–4 mol L–1 min–1
The rate equation for the reaction 2A+B→C is found to be:
rate = k [A] [B]
The correct statement in relation to this reaction is that the:
| 1. | Unit of k must be s-1 |
| 2. | t1/2 is a constant |
| 3. | Rate of formation of C is twice the rate of disappearance of A |
| 4. | Value of k is independent of the initial concentrations of A and B |
For the reaction, 2A → B, rates= k[A]2. If the concentration of reactant is doubled, then the:
| (a) | rate of reaction will be doubled. |
| (b) | rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. |
| (c) | rate constant will change since the rate of reaction and rate constant are directly proportional to each other. |
| (d) | rate of reaction will increase by four times. |
Identify the set of correct statements & choose the correct answer from the options given below:
| 1. | (a) and (c) only | 2. | (a) and (b) only |
| 3. | (b) and (d) only | 4. | (c) and (d) only |
The rate constant for a reaction of zero-order in A is 0.0030 mol L-1 s-1. How long will it take for the initial concentration of A to fall from 0.10 M to 0.075 M?
1. 8.3 sec
2. 0.83 sec
3. 83 sec
4. 10.3 sec
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Q. No.
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