- 1(current)
Q. No.
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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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 |
Level 3: 35%-60%
JEE
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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 |
Level 3: 35%-60%
Hints
The activation energy for the reaction 2HI(g) → H2 + I2(g) is 209.5 kJ mol−1 at 581K. The fraction of molecules of reactants having energy equal to or greater than activation energy is-
1. 2.67 × 10−19
2. 3.57 × 10−18
3. 4.67 × 10−17
4. 1.47 × 10−19
1. 2.67 × 10−19
2. 3.57 × 10−18
3. 4.67 × 10−17
4. 1.47 × 10−19
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
Hints
Consider the given two statements:
| Assertion(A): | The active complex is an intermediate product. |
| Reason(R): | The active complex is unstable because of high energy. |
| 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 but (R) is False. |
| 4. | (A) is False but (R) is True. |
Subtopic: Arrhenius Equation |
Level 4: Below 35%
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For reaction \(A \longrightarrow B,\) the rate constant \(k_1=A_1 e^{-E a_1 /(R T)}\) and
for the reaction \(X \longrightarrow Y \text {, }\)the rate constant \(k_2=A_2 e^{-E a_2 /(R T)}.\)
If \(A_1=10^8, A_2=10^{10}\) and \(E_{a_1}=600~ \mathrm{cal} / \mathrm{mol},\) \(E_{a_2}=1800~ \mathrm{cal} / \mathrm{mol},\)
then the temperature at which \(k_1=k_2\) is:\(\text { (Given : } R=2 \mathrm{cal} / \mathrm{K}-\mathrm{mol} \text { ) }\)
for the reaction \(X \longrightarrow Y \text {, }\)the rate constant \(k_2=A_2 e^{-E a_2 /(R T)}.\)
If \(A_1=10^8, A_2=10^{10}\) and \(E_{a_1}=600~ \mathrm{cal} / \mathrm{mol},\) \(E_{a_2}=1800~ \mathrm{cal} / \mathrm{mol},\)
then the temperature at which \(k_1=k_2\) is:\(\text { (Given : } R=2 \mathrm{cal} / \mathrm{K}-\mathrm{mol} \text { ) }\)
| 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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