Q. No.| Column I: |
Column II: |
||
| (A) | Zero order | (i) | \(k=Ae^{-E_a/RT}\) |
| (B) | First order | (ii) |  |
| (C) | Endothermic reaction | (iii) | \( k=\frac{2.303}{t} \log \frac{[A]_0}{[A]} \) |
| (D) | Arrhenius equation | (iv) | \( k=\frac{1}{t}\left([A]_0-[A]\right)\) |
1. (A) →(iv), (B)→(iii), (C) →(ii), (D)→ (i)
2. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
3. (A) →(ii), (B)→(iii), (C) →(iv), (D)→ (i)
4. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
Which of the following expressions correctly represents this relationship?
1. \(k=Ae^{E_a/RT}\)
2. \(k=Ae^{-E_a/RT}\)
3. \(k=Ae \times {E_a \over RT}\)
4. \(k=Ae \times {RT \over E_a}\)
1. \(k \,\, = A\, \, e^{\frac{-E_{a}}{RT}}\)
2. \(k \,\, = A\, \, e^{\frac{RT}{-E_{a}}}\)
3. \(k \,\, = A\, \, e^{\frac{E_{a}}{RT}}\)
4. None of the above
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1. \(k ~\text {vs}~ T\)
2. \(k~ \text{vs} ~\mathrm{l} / T\)
3. \(\ln k ~\text {vs}~ T\)
4. \(\ln k ~ \text{vs}~ 1 / T\)
Which of the following is affected by the presence of a catalyst in a chemical reaction?
1. Acivation energy
2. Equilibrium concentration
3. Heat of reaction
4. Final products
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| 1. | Reactants don't need to collide to react. |
| 2. | A reaction will only occur if reactants collide in specific orientations. |
| 3. | A reaction can occur when reactants collide in any direction. |
| 4. | A reaction will always occur when reactants collide. |
The temperature dependence of the rate constant (k) of a chemical reaction is written in terms of the Arrhenius equation,
k = A.e–E*/RT. The activation energy (E*) of the reaction can be calculated by plotting:
1.
2.
3.
4.
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Which of the following statements is correct regarding the equation k = Ae-Ea/RT ?
1. k is the equilibrium constant
2. A is adsorption factor
3. Ea is the energy of activation
4. R is the Rydberg constant
| 1. | In K vs T |
| 2. | In \(\frac K T\) vs T |
| 3. | In K vs \(\frac 1 T\) |
| 4. | In \(\frac T K\) vs \(\frac 1 T\) |
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Consider the equilibrium reaction: A(g) ⇌ B(g) with an enthalpy change (ΔH) of -42 kJ/mol.
Determine the activation energies for the forward and backward reactions, given that the ratio of the activation energy of the forward reaction to the activation energy of the backward reaction is 2 : 3.
| 1. | 84 kJ/mole, 126 kJ/mole | 2. | 24 kJ/mole, 36 kJ/mole |
| 3. | 48 kJ/mole, 72 kJ/mole | 4. | 90 kJ/mole, 135 kJ/mole |
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