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)
as described by the Arrhenius equation, is:
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
1. \(k ~\text {vs}~ T\)
2. \(k~ \text{vs} ~\mathrm{l} / T\)
3. \(\ln k ~\text {vs}~ T\)
4. \(\ln k ~ \text{vs}~ 1 / T\)
The effect of a catalyst in a chemical reaction is to change the
1. Acivation energy.
2. Equilibrium concentration.
3. Heat of reaction.
4. Final products.
| 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.
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 \(\frac 1 T\) |
The activation energy of a reaction can be determined from the slope of the graph between :
1. ln K vs T
2. ln vs T
3. ln K vs
4.
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