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]
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. |
The unit of rate constant for a zero-order reaction is:
1.
2.
3.
4.
The rate of the reaction can be written in three ways:
The relationship between k and k′ and between
k and k′′ are-
1. k′ = k, k′′= k
2. k′= 2k; k′′= k
3. k′= 2k, k′′= k/2
4. k′ = 2k; k′′= 2k
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 rate of the reaction
2NO + Cl2 → 2NOCl is given by the rate equation
rate = k[NO]2[Cl2]
The value of the rate constant can be increased by:
1. Increasing the concentration of NO
2. Increasing the concentration of Cl2
3. Increasing the temperature
4. All of the above
The half-life period of a first-order reaction is 1386 s. The specific rate constant of the reaction is:
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2.
3.
4.
For the reaction, A + B → products, it is observed that-
(1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
(2) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is given by:
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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:
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