Consider the following values of rate constant:
(i) k = 2.3 × 10–5 L mol–1 s–1
(ii) k = 3 × 10–4 s–1
The correct statement among the following is-
1. | The order for (i) is second order and the order for (ii) is first order. |
2. | The order for (i) is zero order and the order for (ii) is first order. |
3. | The order for (i) is second order and the order for (ii) is zero order. |
4. | The order for (i) is first order and the order for (ii) is zero order. |
The initial concentration of N2O5 in the following first-order reaction N2O5(g) → 2 NO2(g) + 1/2 O2 (g) was 1.24 × 10–2 mol L–1 at 318 K. The concentration of N2O5 after 60 minutes was 0.20 × 10–2 mol L–1. The rate constant value at 318 K is-
1. 0.304 min-1
2. 0.00304 min-1
3. 0.0304 min-1
4. 3.04 min-1
The following data were obtained during the first order thermal decomposition of N2O5 (g) at constant volume:
S.NO. | Time/s | Total Pressure/(atm) |
1 | 0 | 0.5 |
2 | 100 | 0.512 |
The rate constant value is-
1. \(5.98\times 10^{-4}\) sec–1
2. \(4.98\times 10^{-4}\) sec–1
3. \(6.98\times 10^{-4}\) sec–1
4. \(7.98\times 10^{-4}\) sec–1
A first-order reaction is found to have a rate constant, k = 5.5 × 10–14 s–1. The half-life of the reaction is-
1. | 1.66 × 1013 s |
2. | 1.46 × 1013 s |
3. | 1.36 × 1013 s |
4. | 1.26 × 1013 s |
In a first order reaction, time required for completion of 99.9% is X times of half-life (t1/2) of the reaction. When reaction is completed 99.9%, [R]n = [R]0 – 0.999[R]0 .The value of X is-
1. 5
2. 10
3. 15
4. 20
The rate constants of a reaction at 500K and 700K are 0.02s–1 and 0.07s–1 respectively. The values of Ea is-
1. 15.6 kJ
2. 13.7 kJ
3. 18.2 kJ
4. 17.5 kJ