1 mole of a gas changes linearly from its initial state (2 atm, 10 lt) to its final state (8 atm, 4 lt). The maximum rate constant is equal to 20 and the value of activation energy is 40 kJ, assuming that the activation energy does not change in this temperature range. The value of the rate constant, at the maximum temperature that the gas can attain, is:
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2.
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4.
A first-order reaction was started with a decimolar solution of the reactant. After 8 minutes and 20 seconds, its concentration was found to be M/100. The rate constant of the reaction will be:
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The decomposition of A into product has value of k as \(4.5 \times 10^3 \mathrm{~s}^{-1} \text { at } 10^{\circ} \mathrm{C}.\) Energy of activation of the reaction is \(60 \mathrm{~kJ}~mol^{-1}.\) The temperature at which value k would become \(1.5\times10^4~s^{-1}\) is :
1. | \(12{ }^{\circ} \mathrm{C} \) | 2. | \(24^{\circ} \mathrm{C} \) |
3. | \(48^{\circ} \mathrm{C} \) | 4. | \(36^{\circ} \mathrm{C}\) |
For the reaction 2N2O5(g) → 4NO2(g) + O2(g)the concentration of increases by 2.4 × 10-2 mol L-1
in 6 seconds. The rate of appearance of and the rate of disappearance of , respectively, are:
1. 2 x 10-3 mol L-1 sec-1, 4 x 10-3 mol L-1 sec-1
2. 2 x 10-3 mol L-1 sec-1, 1 x 10-3 mol L-1 sec-1
3. 2 x 10-3 mol L-1 sec-1, 2 x 10-3 mol L-1 sec-1
4. 4 x 10-3 mol L-1 sec-1, 2 x 10-3 mol L-1 sec-1
The rate constant of a particular reaction has the dimension of frequency. The order of the reaction is:
1. Zero.
2. First.
3. Second.
4. Fractional.
For the reaction, C2H5I + OH- → C2H5OH + I- the rate constant was found to have a value of 5.03 × 10-2 moI-1 dm3 s-1 at 289 K and 6.71 mol-1 dm3 s-1 at 333 K.
The rate constant at 305 K will be:
The first order rate constant for a certain reaction increases from\(1.667 \times 10^{-6} \mathrm{~s}^{-1} \text { at } 727^{\circ} \mathrm{C} \text { to } 1.667 \times 10^{-4} \mathrm{~s}^{-1} \text { at } 1571{ }^{\circ} \mathrm{C}.\) The rate constant at \(1150^{\circ} \mathrm{C}\) is:
(assume activation energy is constant over the given temperature range)
1. | \(3.911 \times 10^{-5} \mathrm{~s}^{-1} \) | 2. | \(1 .139 \times 10^{-5} \mathrm{~s}^{-1} \) |
3. | \(3.318 \times 10^{-5} s^{-1} \) | 4. | \(1.193 \times 10^{-5} \mathrm{~s}^{-1}\) |
The thermal decomposition of a compound is of first order. If 50 % of a sample of the compound decomposes in 120 minutes, how long will it take for 90 % of the compound to decompose?
1. 399 min
2. 410 min
3. 250 min
4. 120 min
The half-life for radioactive decay of is 5730 y. An archaeological artifact containing wood had only 80 % of the found in a living tree. The age of the sample will be:
1. 1657.3 y
2. 1845.4 y
3. 1512.4 y
4. 1413.1 y
The following data were obtained during the first-order thermal decomposition of at a constant volume.
SO2Cl2(g) → SO2(g) + Cl2(g)
Experiment | Time/s | Total pressure/atm |
1 | 0 | 0.5 |
2 | 100 | 0.6 |
The rate of the reaction when total pressure is 0.65 atm will be:
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