The rate of the reaction, 2NO + Cl2 $$ \to $$ 2NOCl is given by the rate equation rate = k[NO]2[Cl2]. The value of the rate constant can be increased by
A
increasing the temperature
B
increasing the concentration of NO
C
increasing the concentration of the Cl2
D
doing all of these.
Explanation
The value of rate constant can be increased by
increasing the temperature and is independent
of the initial concerntration of the reactants.
2
AIPMT 2010 Prelims
MCQ (Single Correct Answer)
For the reaction N2O5(g) $$ \to $$ 2NO2(g) + 1/2O2(g) the value of rate of disappearance of N2O5 is given as 6.25 $$ \times $$ 10$$-$$3 mol L$$-$$1 s$$-$$1. The rate of formation of NO2 and O2 is given respectively as
Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is
A
0.5 $$ \times $$ 10$$-$$2 s$$-$$1
B
0.5 $$ \times $$ 10$$-$$3 s$$-$$1
C
5.0 $$ \times $$ 10$$-$$2 s$$-$$1
D
5.0 $$ \times $$ 10$$-$$3 s$$-$$1.
Explanation
Specific rate constant
k = $${{0.693} \over {{t_{1/2}}}}$$
= $${{0.693} \over {1386}}$$
= 0.5 $$ \times $$ 10-3 sec-1
4
AIPMT 2009
MCQ (Single Correct Answer)
For the reaction A + B $$ \to $$ products, it is observed that
(i) on doubling the initial concentration of A only, the rate of reaction is also doubled and
(ii) on doubling the initial concentration 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
A
rate = k[A]2 [B]2
B
rate = k[A] [B]2
C
rate = k[A] [B]
D
rate = k[A]2 [B]
Explanation
R = k[A]m[B]n
... (i)
2R = k[2A]m[B]n
... (ii)
8R = k[2A]m[2B]n
... (iii)
from (i), (ii) and (iii), m = 1, n = 2
So, rate = k[A][B]2
Questions Asked from Chemical Kinetics
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