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 ° 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
The incorrect statement regarding the order of reaction is:
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 |
[B)/ mol L |
Initial rate of L |
I |
0.1 |
0.1 |
6.0 |
II |
0.3 |
0.2 |
7.2 |
III |
0.3 |
0.4 |
2.88 |
IV |
0.4 |
0.1 |
2.40 |
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.
For the reaction, \(\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3,\) if, \(\frac{d[NH_{3}]}{dt} \ = \ 2\times 10^{-4} \ mol \ L^{-1} \ s^{-1}\), the value of \(\frac{-d[H_{2}]}{dt}\) would be:
1. | \(3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) | 2. | \(4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) |
3. | \(6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) | 4. | \(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) |
In the reaction,
3Br2(l)+3H2O(l)
The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions:
1.
2.
3.
4.