Q. No.When the initial concentration of the reactant is doubled,
the half-life period of a zero-order reaction:
1.
is halved
2.
is doubled
3.
is tripled
4.
remains unchanged
the half-life period of a zero-order reaction:
| 1. | Internal energy | 2. | Enthalpy |
| 3. | Activation energy | 4. | Entropy |
1. 44.1 s
2. 54.1 s
3. 24.1 s
4. 34.1 s
The rate Constant of reaction A → B is 0.6 × 10–3 \(\mathrm{molL}^{-1} \mathrm{~S}^{-1}\). If the Concentration of A is 5M, then the concentration of B after 20 min is:
1. 1.08M
2. 3.60M
3. 0.36M
4. 0.72M
2. ln vs T
3. ln K vs
4. ln
When the initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction will be:
1. 0
2. 1
3. 1.5
4. 2
| 1. | 269 kJ mol–1 | 2. | 34.7 kJ mol–1 |
| 3. | 15.1 kJ mol–1 | 4. | 342 kJ mol–1 |
A reaction having equal energies of activation for forward and reverse reaction has:
1. ΔG = 0
2. ΔH = 0
3. ΔH = ΔG = ΔS = 0
4. ΔS = 0
In a reaction, A + B → Product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8, when the concentrations of both the reactants (A and B) are doubled. The rate law for the reaction can be written as:
1. Rate = k[A][B]2
2. Rate = k[A]2[B]2
3. Rate = k[A][B]
4. Rate = k[A]2[B]
In a zero-order reaction for every 10 °C rise of temperature, the rate is doubled.
If the temperature is increased from 10 °C to 100 °C, the rate of the reaction will become:
1. 256 times
2. 512 times
3. 64 times
4. 128 times
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