Acid catalysed hydrolysis of ethyl acetate follows a pseudo-first order kinetics with respect to ester. If the reaction is carried out with large excess of ester, the order with respect to ester will be
1.5
0
0.5
1
The half-life for decay of 14C by β-emission is 5730 yr. The fraction of 14C decays, in a sample that is 22920 yr old, would be
A piece of wood from an archaeological sample has 5.0 counts min-1 per gram of C-14, while a fresh sample of wood has a count of 15.0 min-1g-1. If half-life of C-14 is 5770 yr, the age of the archaeological sample is
8,500 yr
9,200 yr
10,000 yr
11,000 yr
Consider the following reaction for 2NO2(g) + F2(g) → 2NO2Fg). The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are
rate =
rate =
rate =
rate =
The bacterial growth follows the rate law, = kN where k is a constant and 'N' is the dt number of bacteria cell at any time. If the population of bacteria (number of cell) is doubled in 5 min find the time in which the population will be eight times of the initial one?
As ( It is a first order reaction)
Integrated rate equation for Ist order reaction
k =
when t = 5 min; N = 2N0
k =
or, k =
For N = 8N0 ; t = ?
t =
By putting the value of k
t =
or, t = = 15 min
following mechanism has been provided.
Thus, rate expression of the above reaction can be written as
r =k [NO2]2[F2]
r= k [NO2] [F2]
r= k [NO2]
r= k [F2]
For a reaction, an aqueous medium, the rate of reaction is given by:
The overall order of reaction is
-1
0
1
2
Reaction between compounds (A) and (B) occurs as follows
A (g) + 2B (g) → 2C (g)
Following results were obtained
(1) Exp. No. | (2) Initial concentration of [A] mol L-1 | (3) Initial concentration of [B] mol L-1 | (4) Initial rate of formation of [C] mol L-1 s-1 |
1. | 0.30 | 0.30 | 0.10 |
2. | 0.30 | 0.60 | 0.40 |
3. | 0.60 | 0.30 | 0.20 |
The correct rate- law for the said reaction is (r and k rate and rate constant respectively)
r = k[A]2B
r = k[A][B]2
r = k[A][B]
r = k[A]2[B]2
In the reaction 2NO2 N2O4; the rate of disappearance of NO2 is equal to
2 [NO2]2
2k1[NO2]2 - 2k2[N2O4]
2k2[NO2]2 - k2[N2O4]
(2k1 - k2)[NO2]
The rate constant for the raection 2N2O5 → 4NO2 + O2 is 3.0 × 10-5 s-1. If rate is 2.40 × 10-5, then concentration of N2O5 (in mol/L) is
1.4
1.2
0.04
0.8