CBSE
The unit of rate constant for a zero order reaction is
mol L-1 s-1
L mol-1 s-1
L2 mol-2 s-1
L2 mol-2 s-1
For the reaction
the value of the rate of disappearance of N2O5 is given as
6.25 x 10-3 mol L-1s-1 and 6.25 x 10-3 mol L-1 s-1
1.25 x 10-2 mol L-1s-1 and 6.25 x 10-3 mol L-1 s-1
6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1 s-1
6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1 s-1
For the reaction, A+B → Products, it is observed that
1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
2) On doubling the initial concentrations of both A and B , there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is, given by
rate = k [A]2[B]
rate = k[A][B]2
rate = k[A]2[B]2
rate = k[A]2[B]2
The rate of reaction 2N2O3 → 4 NO2 + O2 can be written in three ways
The relationship between k and k' and between k and k'' are
k' = 2k ; k' = k
k' = 2k; k" = k/2
k' = 2k; k' = 2k
k' = 2k; k' = 2k
Half-life period of a first order reaction is 1386 s. The specific rate constant of the reaction is
5.0 x 10-3s-1
0.5 x 10-2 s-1
0.5 x 10-3 s-1
0.5 x 10-3 s-1
During the kinetic study of the reaction, 2A + B --> C+ D, following results were obtained
|
[A]/mol L- |
[B]/ mol L- |
Initial rate of formation of D/ mol L- min- |
I |
0.1 |
0.1 |
6.0 x 10-3 |
II |
0.3 |
0.2 |
7.2 x 10-2 |
III |
0.3 |
0.4 |
2.88 x 10-1 |
IV |
0.4 |
0.1 |
2.40 x10-2 |
rate = k[A]2[B]
rate = k [A][B]
rate = k[A]2[B]2
rate = k[A]2[B]2
For an endothermic reaction, energy of activation is Ea and enthalpy of reaction is ΔH (both of these in kJ/mol). Minimum value of Ea will be
less than ΔH
equal to ΔH
more than ΔH
more than ΔH
The rate of constant of the reaction A → B is 0.6 x 10-3 mole per second. If the concentration of A is 5 M then concentration of B after 20 min is
1.08 M
3.60 M
0.36 M
0.36 M
The half -life of a substance in a certain enzyme catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L-1 is
414 s
552 s
690 s
690 s
The rate of the reaction,
2NO + Cl2 → 2NOCl is given by the rate equation, rate = k[NO]2[Cl2]
The value of the rate constant can be increased by
increasing the temperature
increasing the concentration of NO
increasing the concentration of the Cl2
increasing the concentration of the Cl2