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 \(\mathrm{mol} \text { litre }{ }^{-1}\) 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 , at the point of intersection of two curves show, the [B] is can be given by:
1.
2.
3.
4.
The rate constant of a first-order reaction is\(4 \times 10^{-3} \mathrm{sec}^{-1}.\) At a reactant concentration of \(0.02~\mathrm{M},\) the rate of reaction would be:
1. | \(8 \times 10^{-5} \mathrm{M} ~\mathrm{sec}^{-1} \) | 2. | \(4 \times 10^{-3} \mathrm{M} ~\mathrm{sec}^{-1} \) |
3. | \(2 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1} \) | 4. | \(4 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1}\) |
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
It means:
1. Rate constant of overall reaction is 4 sec-1
2. Rate of reaction is independant of the concentration of acid
3. The change in pH of the solution will not affect the rate
4. Doubling the conc. of H+ ions will increase the reaction rate by 4 times
A graph plotted between log (t) 50% vs. log (a) concentration is a straight line. What conclusion can you draw from the given graph?
1. n=1, t1/2 = 1/K.a
2. n=2, t1/2 = 1/a
3. n=1, t1/2 = 0.693/K
4. None of the above