For the reaction:
[Cu(NH3)4]2+ + H2O⇌[Cu(NH3)3H2O]2+ + NH3
the net rate of reaction at any time is given by, net rate =
2.0x10-4 [Cu(NH3)4]2+[H2O] - 3.0x105 [Cu(NH3 )3 H20]2+[NH3]
Then correct statement is/are :
1. rate constant for forward reaction = 2 x 10-4
2. rate constant for backward reaction = 3 x 105
3. equilibrium constant for the reaction = 6.6 x 10-10
4. all of the above
Rate constant of reaction can be expressed by Arrhenius equation as,
K=Ae-EaRT
In this equation, Ea represents:
1. the energy above which all the colliding molecules will react
2. the energy below which colliding molecules will not react
3. the total energy of the reacting molecules at a temperature, T
4. the fraction of molecules with energy greater than the activation energy of the reaction
Consider the chemical reaction,
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) and NH3(g).
The correct relationship amongest the rate expressions is:
(1) Rate =-d[N2]dt=-13 d[H2]dt=12 d[NH3]dt
(2) Rate =-d[N2]dt=-3 d[H2]dt=2 d[NH3]dt
(3) Rate =d[N2]dt=13 d[H2]dt=12 d[NH3]dt
(4) Rate =-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 −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 |