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Q. No.The activation energy of one of the reactions in a biochemical process is \(\mathrm{532611~ J~ mol^{–1} .}\) When the temperature falls from \(\mathrm{310~ K}\) to \(\mathrm{300~ K,}\) the change in rate constant observed is \(\mathrm{k_{300} = x × 10^{–3} k_{310}.}\)
The value of \(\mathrm{x}\) is:
[Given: ln\(\mathrm{10 = 2.3, R = 8.3 ~JK^{–1} mol^{–1}}\) ]
1.
1
2.
5
3.
2
4.
8
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
JEE
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Consider the given reaction:
\(A(g) \xrightarrow{k=0.1 M \min ^{-1}} 2 B(\mathrm{~g}) \)
If the initial concentration of A is 0.5 M, which of the following graphs correctly represents the concentration of B over time?
\(A(g) \xrightarrow{k=0.1 M \min ^{-1}} 2 B(\mathrm{~g}) \)
If the initial concentration of A is 0.5 M, which of the following graphs correctly represents the concentration of B over time?
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2 |  |
| 3 |  |
4 |  |
Subtopic: Definition, Rate Constant, Rate Law |
Level 3: 35%-60%
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Consider the graph [between half-life \(\left(t_{1 / 2}\right)\) and initial concentration (a) of the reactant] for the reaction \(A \longrightarrow B,\)
The graph between \(-\dfrac{d[A]}{d t}\) and time will be:
The graph between \(-\dfrac{d[A]}{d t}\) and time will be:
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2 |  |
| 3 |  |
4 |  |
Subtopic: Order, Molecularity and Mechanism |
51%
Level 3: 35%-60%
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The rate of reaction will be fast if:
1. \(\Delta G^\circ\) is a large negative number
2. \(\Delta S^\circ\) is a large negative number
3. \(\Delta H^\circ\) is a large negative number
4. None of the above can be used to estimate reaction rates.
1. \(\Delta G^\circ\) is a large negative number
2. \(\Delta S^\circ\) is a large negative number
3. \(\Delta H^\circ\) is a large negative number
4. None of the above can be used to estimate reaction rates.
Subtopic: Definition, Rate Constant, Rate Law |
54%
Level 3: 35%-60%
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A catalyst will not:
| 1. | Increase the forward reaction rate. |
| 2. | Shift the equilibrium to favor the products. |
| 3. | Alter the reaction pathway. |
| 4. | Increase the speed at which equilibrium will be achieved. |
Subtopic: Catalyst |
54%
Level 3: 35%-60%
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The Arrhenius equations for two reactions are:
A → B: k₁ = 10⁸ exp(−600/RT)
X → Y: k₂ = 10¹⁰ exp(−1800/RT)
The temperature (in Kelvin) at which k₁ = k₂ is:
(Given R = 2 cal mol⁻¹ K⁻¹)
| 1. | \(1200 \mathrm{~K}\) | 2. | \(1200 \times 4.606 \mathrm{~K}\) |
| 3. | \(\dfrac{1200}{4.606} \mathrm{~K}\) | 4. | \(\dfrac{600}{4.606} \mathrm{~K}\) |
Subtopic: Arrhenius Equation |
59%
Level 3: 35%-60%
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Two first-order reactions have half-lives in the ratio \(8:1.\) Calculate the ratio of the time intervals \(t_1: t_2\)where the time \(t_1\) and \(t_2\) are the time periods for \(\left(\frac{1}{4}\right)^{\mathrm{th}}\) and \(\left(\frac{3}{4}\right)^{\mathrm{th}}\) completion of the reaction, respectively.
1. \(1: 0.301\)
2. \(0.125: 0.602\)
3. \(1: 602\)
4. None of the above
1. \(1: 0.301\)
2. \(0.125: 0.602\)
3. \(1: 602\)
4. None of the above
Subtopic: First Order Reaction Kinetics |
Level 4: Below 35%
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The forward rate constant for an elementary reversible gaseous reaction is given as
\(\mathrm{C}_2 \mathrm{H}_6 \rightleftharpoons 2 \mathrm{CH}_3 \text { is } 1.57 \times 10^{-3} \mathrm{~s}^{-1} \text { at } 100 \mathrm{~K}\)
What is the rate constant for the backward reaction at this temperature if \(10^{-4}\) moles of \(\mathrm{CH}_3\) and \(10\) moles of \(\mathrm{C}_2 \mathrm{H}_6\) are present in a \(10\) litre vessel at equilibrium?
1. \(1.57 \times 10^9 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
2. \(1.57 \times 10^{10} \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
3. \(1.57 \times 10^{11} \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
4. \(1.57 \times 10^7 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
Subtopic: Definition, Rate Constant, Rate Law |
66%
Level 2: 60%+
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Which of the following statements is/are Incorrect?
1. i only
2. i and ii only
3. ii and iii only
4. iii only
| (i) | A catalyst lowers the activation energy of a reaction. |
| (ii) | A catalyst allows the same rate of reaction to be achieved at a lower temperature. |
| (iii) | A catalyst mixes with the reactants and increases the overall concentration of reactants in the rate equation. |
2. i and ii only
3. ii and iii only
4. iii only
Subtopic: Catalyst |
Level 3: 35%-60%
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Which of the following statements is true regarding the nature of reaction order and reaction mechanisms?
| 1. | A second-order reaction is always a multistep reaction. |
| 2. | A zero-order reaction is a multistep reaction. |
| 3. | A first-order reaction is always a single-step reaction. |
| 4. | A zero-order reaction is a single-step reaction. |
Subtopic: Order, Molecularity and Mechanism |
Level 3: 35%-60%
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