The incorrect statement among the following is:
1.
The value of the equilibrium constant is changed in the presence of a catalyst in the reaction at equilibrium
2.
Enzymes catalyse mainly bio-chemical reactions
3.
Coenzymes increase the catalytic activity of the enzyme
4.
The catalyst does not initiate any reaction
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 |
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
Which of the following statements about the order of reaction is incorrect?
| 1. | Order is not influenced by the stoichiometric coefficient of the reactants. |
| 2. | Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction. |
| 3. | The order of reaction is always a whole number. |
| 4. | Order can be determined by experiments only. |
During the kinetic study of the reaction, 2A + B\( \rightarrow\)C + D, following results were obtained:
| Run | [A)/ mol L-1 | [B)/ mol L-1 | Initial rate of formation of D/mol L-1 |
| I | 0.1 | 0.1 | \(6.0 \times 10^{- 3}\) |
| II | 0.3 | 0.2 | \(7.2 \times 10^{- 2}\) |
| III | 0.3 | 0.4 | \(2.88 \times \left(10\right)^{- 1}\) |
| IV | 0.4 | 0.1 | \(2.40 \times \left(10\right)^{- 2}\) |
Based on the above data which one of the following is correct?
1. rate= k[A]2[B]
2. rate= k[A][B]
3. rate= k[A]2[B]2
4. rate= k[A][B]2
The half-life period of a first-order reaction is 1386 s. The specific rate constant of the reaction is:
1.
2.
3.
4.
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