Q. No.Consider the two rate laws:
(I) Rate = k [A]1/2 [B]3/2
(II) Rate = k [A]3/2 [B]–1
The correct statement among the following is-
| 1. | The overall order for rate expression (I) is 2 and for (II) is \(\frac{5}{2}\) |
| 2. | The overall order for rate expression (I) is 2 and for (II) is \(\frac{1}{2}\) |
| 3. | The overall order for rate expression (I) is -2 and for (II) is \(\frac{3}{2}\) |
| 4. | The overall order for rate expression (I) is -2 and for (II) is \(\frac{5}{2}\) |
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In the reaction: \(\small {\mathrm{A}+2 \mathrm{~B} \rightarrow 6 \mathrm{C}+2 \mathrm{D},}\) if the initial rate \(-\dfrac{d[A]}{d t}\) at \(t=0\) is \(2.6 \times 10^{-2} \mathrm{M} \mathrm{~sec}^{-1},\) then find the value of \(-\dfrac{d[B]}{d t} \text { at } t=0 \):
| 1. | \(8.5 \times 10^{-2} \mathrm{M} \mathrm~\text{sec}^{-1}\) | 2. | \(2.5 \times 10^{-2} \text M \sec ^{-1}\) |
| 3. | \(5.2 \times 10^{-2} \mathrm{M} \mathrm{~sec}^{-1}\) | 4. | \(7.5 \times 10^{-2} \mathrm{M} \mathrm{~sec}^{-1}\) |
In a reaction, the rate expression is, rate = K[A][B]2/3[C]0, the order of the reaction is:
1. 1
2. 2
3. 5/3
4. zero
The reaction 2A + B + C D + E is found to be a first-order reaction with respect to A, second-order reaction with respect to B, and zero-order reaction with respect to C. If the concentrations of A, B, and C are doubled, the rate of the reaction will be:
1. 72 times
2. 8 times
3. 24 times
4. 36 times
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(Given: Co = Initial concentration of reactant)
| 1. | \(\frac{[C_0]}{k} \) | 2. | \(\frac{[C_0]}{2 k} \) |
| 3. | \(\frac{[2 C_0]}{k} \) | 4. | \(\frac{[2 C_0]}{3 k}\) |
| 1. | \(k[A][B][C]^{0.5}\) | 2. | \(k[A]^{0.5}[B]^{0.5}[C]^{0.5}\) |
| 3. | \(k[A]^{1.5}[B]^{-1}[C]^0\) | 4. | \(k[A][B]^0[C]^{0.5}\) |
1. \( r=k[A]^{\frac{1}{2}}[B]^1 \)
2. \( \mathrm{r}=\mathrm{k}[\mathrm{A}]^{\frac{1}{2}}[\mathrm{~B}]^{-1} \)
3. \( r=k[A]^{\frac{3}{2}}[B]^{\frac{1}{2}} \)
4. \( r=k[A]^{-\frac{1}{2}}[B]^{\frac{3}{2}}\)
A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will:
1. Remain unchanged
2. Triple
3. Increases by a factor of 4
4. Double
If the rate of the reaction is equal to the rate constant, the order of the reaction is:
| 1. | 0 | 2. | 1 |
| 3. | 2 | 4. | 3 |
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The rate law for a reaction is rate = k[A]²[B]. If the concentrations of both A and B are doubled, the rate becomes x times the original rate, and the overall order of the reaction is y. The value of (x + y) is:
| 1. | 11 | 2. | 87 |
| 3. | 67 | 4. | 20 |
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