The correct statement among the following is:
1. | the rate of a first-order reaction does not depend on reactant concentration; the rate of a second-order reaction does depend on reactant concentrations. |
2. | the half-life of a first-order reaction does not depend on [A]o; the half-life of a second-order reaction does depend on [A]0 |
3. | a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed. |
4. | the rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations |
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 |
1. | Internal energy | 2. | Enthalpy |
3. | Activation energy | 4. | Entropy |
The rate Constant of reaction A B is 0.6 × 10–3 mole per second. If the Concentration of A is 5, then the concentration of B after 20 min is:
1. 1.08M
2. 3.60M
3. 0.36M
4. 0.72M
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
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]