1. | Rate=k[A]0[B]2 | 2. | Rate=k[A][B] |
3. | Rate=k[A]1/2[B]2 | 4. | Rate=k[A]−1/2[B]3/2 |
1. | −Δ[A]Δt | 2. | −3Δ[A]2Δt |
3. | −2Δ[A]3Δt | 4. | Δ[A]Δt |
1. | Increase by a factor of three |
2. | Decrease by a factor of nine |
3. | Increase by a factor of six |
4. | Increase by a factor of nine |
Assertion (A): | A reaction can have zero activation energy. |
Reason (R): | The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation 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. |
1. | 1 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
2. | 10 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
3. | 1 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
4. | 10 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
The plot of ln k vs 1T for the following reaction
2N2O5(g)→4NO2(g)+O2(g) gives a straight line with the slope of the line equal to −1.0×104K.
The activation energy for the reaction in J mol–1 is:
(Given R = 8.3 J K–1 mol–1)
1. | 4.0×102 | 2. | 4.0×10−2 |
3. | 8.3×10−4 | 4. | 8.3×104 |
For the reaction, 2A → B, rates= k[A]2. If the concentration of reactant is doubled, then the:
(a) | rate of reaction will be doubled. |
(b) | rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. |
(c) | rate constant will change since the rate of reaction and rate constant are directly proportional to each other. |
(d) | rate of reaction will increase by four times. |
Identify the set of correct statements & choose the correct answer from the options given below:
1. | (a) and (c) only | 2. | (a) and (b) only |
3. | (b) and (d) only | 4. | (c) and (d) only |