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Q. No.The decomposition of a gaseous compound yields the following information:
| Initial pressure, atm | 1.6 | 0.8 | 0.4 |
| Time for 50 % reaction, min | 80 | 113 | 160 |
| 1. | 1.0 | 2. | 1.5 |
| 3. | 2.0 | 4. | 0.5 |
Subtopic: Definition, Rate Constant, Rate Law |
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| Assertion(A): | For exothermic reaction equilibrium constant decreases with an increase in temperature. |
| Reason(R): | For a reaction, the rate constant decreases with decrease in temperature. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True and (R) is False |
| 4. | (A) is False and (R) is True |
Subtopic: Definition, Rate Constant, Rate Law |
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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?
| 1 |  |
2 |  |
| 3 |  |
4 |  |
Subtopic: Definition, Rate Constant, Rate Law |
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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 |
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For the reaction A + B → C, experiments were performed in the presence of a large amount of B to measure the initial reaction rate (Vf) as a function of the initial concentration of A ([A]0). The data from the experiments are plotted as shown below. The order of the reaction with respect to A is:
1. 1
2. 3
3. 2/3
4. 3/2
1. 1
2. 3
3. 2/3
4. 3/2
Subtopic: Definition, Rate Constant, Rate Law |
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Consider the following reversible reaction
\(\)
(K1 is the rate constant for the forward reaction and K2 is the rate constant for the backward reaction). The rate law for the appearance of NH3 is
\(1.~K_{2}\left[NH_{3}\right]^2 -K_1\left[N_{2}\right][H_2]^{3}\\ 2.~2\mathrm{~K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}-2 \mathrm{~K}_{2}\left[\mathrm{NH}_{3}\right]^{2}\\ 3.~2 \mathrm{~K}_{2}\left[\mathrm{NH}_{3}\right]^{2}-2 \mathrm{~K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}\\ 4.~\mathrm{K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}-\mathrm{K}_{2}\left[\mathrm{NH}_{3}\right]^{2}\)
\(\)
(K1 is the rate constant for the forward reaction and K2 is the rate constant for the backward reaction). The rate law for the appearance of NH3 is
\(1.~K_{2}\left[NH_{3}\right]^2 -K_1\left[N_{2}\right][H_2]^{3}\\ 2.~2\mathrm{~K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}-2 \mathrm{~K}_{2}\left[\mathrm{NH}_{3}\right]^{2}\\ 3.~2 \mathrm{~K}_{2}\left[\mathrm{NH}_{3}\right]^{2}-2 \mathrm{~K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}\\ 4.~\mathrm{K}_{1}\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}-\mathrm{K}_{2}\left[\mathrm{NH}_{3}\right]^{2}\)
Subtopic: Definition, Rate Constant, Rate Law |
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Thermal decomposition of \(Cl_2O_7\) at 400 K in the gaseous phase to \(Cl_2\) and \(O_2\) is a first order reaction with rate constant \(6.932 \times 10^{-3} s^{-1}\). The time (in minutes) required for 90% decomposition of \(Cl_2O_7\) at 400 K is:
1. 5.54
2. 16.61
3. 33.32
4. 332.2
1. 5.54
2. 16.61
3. 33.32
4. 332.2
Subtopic: Definition, Rate Constant, Rate Law |
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Subtopic: Arrhenius Equation |
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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\(\mathrm{10 = 2.3, R = 8.3 ~JK^{–1} mol^{–1}}\) ]
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 |
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What is the pre-exponential factor for a reaction at 500 K with a rate constant of 0.02 s⁻¹ and an activation energy of 18.230 kJ?
1. 1.61
2. 1.41
3. 1.81
4. 1.21
1. 1.61
2. 1.41
3. 1.81
4. 1.21
Subtopic: Arrhenius Equation |
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