Q. No.Consider the chemical reaction,
N2(g)+3H2(g)→2NH3(g)N2(g)+3H2(g)→2NH3(g)
The rate of this reaction can be expressed in terms of time derivative of concentration of N2 (g), H2(g)N2 (g), H2(g) and NH3(g)NH3(g).
The correct relationship amongest the rate expressions is:
(1) Rate =-d[N2]dt=-13 d[H2]dt=12 d[NH3]dt=−d[N2]dt=−13 d[H2]dt=12 d[NH3]dt
(2) Rate =-d[N2]dt=-3 d[H2]dt=2 d[NH3]dt=−d[N2]dt=−3 d[H2]dt=2 d[NH3]dt
(3) Rate =d[N2]dt=13 d[H2]dt=12 d[NH3]dt=d[N2]dt=13 d[H2]dt=12 d[NH3]dt
(4) Rate =-d[N2]dt=- d[H2]dt= d[NH3]dt=−d[N2]dt=− d[H2]dt= d[NH3]dt
For a first order reaction A→→ Product, the initial concentration of A is 0.1 M and after 40 minute it becomes 0.025 M. Calculate the rate of reaction at reactant concentration of 0.01M:
1. 3.47x10-4 M min-1
2. 3.47x10-5 M min-1
3. 1.735 x 10-6 M min-1
4. 1.735 x10-4 M min-1
Select the intermediate in the following reaction mechanism:
O3(g) ⇌⇌ O2(g) +O(g)
O(g) +O3(g) →→ 2O2(g)
1. O3(g)
2. O(g)
3. O2(g)
4. none of these
A reactant with initial concentration 1.386 mol litre −1mol litre −1 showing first order change takes 40 minute to become half. If it shows zero order change taking 20 minute to becomes half under similar conditions, the ratio, K1/K0 for first order and zero order kinetics will be:
1. 0.5 mol-1 litre
2. 1.0 mol/litre
3. 1.5 mol/litre
4. 2.0 mol-1 litre
In a first order reaction, the concentration of the reactant is decreased from 1.0 M to 0.25M in 20 minute. The rate constant of the reaction would be:
1. 10min-1
2. 6.931 min-1
3. 0.6931 min-1
4. 0.06931 min-1
The following mechanism has been proposed for the reaction of NO with Br2 to form NOBr:
NO(g) + Br2(g) ⇌⇌ NOBr2(g)
NOBr2(g) + NO(g) →2NOBr(g)
If the second step is the rate determining step, the order of the reaction with respect to NO(g) will be:
1. 1
2. 0
3. 3
4. 2
For the reaction A →nB, at the point of intersection of two curves show, the [B] is can be given by:
1. nA02
2. A0n-1
3. nA0n+1
4. [n-1n+1]A0
The rate constant of a first-order reaction is4×10−3sec−1. At a reactant concentration of 0.02 M, the rate of reaction would be:
| 1. | 8×10−5M sec−1 | 2. | 4×10−3M sec−1 |
| 3. | 2×10−1M sec−1 | 4. | 4×10−1M sec−1 |
If concentration of reactants is increased by 'X', the rate constant K becomes:
1. eK/X
2. K/X
3. K
4. X/K
In acidic medium the rate of reaction between BrO3- and Br- ions is given by the expression
-d[BrO-3]dt=K[BrO-3][Br-][H+]2
It means:
| 1. | The rate constant of the overall reaction is 4 sec-1. |
| 2. | The rate of reaction is independent of the concentration of the acid. |
| 3. | The change in pH of the solution will not affect the rate. |
| 4. | Doubling the concentration of H+ ions will increase the rate of reaction by 4 times. |
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