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Q. No.For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M in 25 minutes.
The average rate of reaction in M sec–1 is-
1. 6.67×10–5 M s–1
2. 5.67×10–5 M s–1
3. 6.67×10–6 M s–1
4. 5.67×10–6 M s–1
The average rate of reaction in M sec–1 is-
1. 6.67×10–5 M s–1
2. 5.67×10–5 M s–1
3. 6.67×10–6 M s–1
4. 5.67×10–6 M s–1
Subtopic: Definition, Rate Constant, Rate Law |
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In a reaction, 2A → Products, the concentration of A decreases from 0.5 mol L−1 to 0.4 mol L−1 in 10 minutes.
The rate during this interval is-
1. 5×10–3M min–1
2. 8×10–3M min–1
3. 9×10–3M min–1
4. 3×10–3M min–1
The rate during this interval is-
1. 5×10–3M min–1
2. 8×10–3M min–1
3. 9×10–3M min–1
4. 3×10–3M min–1
Subtopic: Definition, Rate Constant, Rate Law |
67%
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For a reaction, A + B → Product; the rate law is given by, r=k[A]1/2[B]2. The order of the reaction is:
| 1. | –1.5 | 2. | 1.5 |
| 3. | 0.5 | 4. | 2.5 |
Subtopic: Order, Molecularity and Mechanism |
78%
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The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times, then the rate of formation of Y will -
| 1. | Decreases by 3 times | 2. | Increase by 3 times |
| 3. | Decreases by 9 times | 4. | Increase by 9 times |
Subtopic: Order, Molecularity and Mechanism |
75%
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A first order reaction has a rate constant 1.15 × 10−3 s−1. The time required to convert 5g of this reactant into 3g is-
1. 424 s
2. 444 s
3. 464 s
4. 484 s
1. 424 s
2. 444 s
3. 464 s
4. 484 s
Subtopic: First Order Reaction Kinetics |
61%
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Time required to decompose SO2Cl2 to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, the rate constant of the reaction in sec–1 is-
| 1. | 1.9 × 10–4 s–1 | 2. | 1.7 × 10–4 s–1 |
| 3. | 2.2 × 10–4 s–1 | 4. | 1.6 × 10–4 s–1 |
Subtopic: First Order Reaction Kinetics |
67%
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Rate constant (k) and temperature (T) are related as :
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. \(k \,\, = A\, \, e^{\frac{-E_{a}}{RT}}\)
2. \(k \,\, = A\, \, e^{\frac{RT}{-E_{a}}}\)
3. \(k \,\, = A\, \, e^{\frac{E_{a}}{RT}}\)
4. None of the above
Subtopic: Arrhenius Equation |
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The rate of the chemical reaction doubles for an increase of 10 K in absolute temperature from 298 K. The value of Ea is-
1. 49.5 kJ mol–1
2. 52.9 kJ mol–1
3. 55.5 kJ mol–1
4. 57.9 kJ mol–1
1. 49.5 kJ mol–1
2. 52.9 kJ mol–1
3. 55.5 kJ mol–1
4. 57.9 kJ mol–1
Subtopic: Arrhenius Equation |
63%
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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 |
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