Kinetics
1. In
32 minutes, 75% of a first order reaction was completed. When was 50% of the
reaction completed:-
a. 24
minutes
b. 16
minutes
c. 8
minutes
d. 4
minutes
2. The
reaction between X and Y is first order with respect to X and second order with
respect to Y. If the concentration of X is halved and the concentration of Y is doubled, the rate of reaction will be:-
a. Same
as initial value
b. Double
the initial value
c. Three
times the initial value
d. Half
the initial value
3. In
the reaction N2 + 3H2→2NH3, the rate of
disappearance of H2 is1.8×10-5mol L-1s-1.
Therefore, the rate of formation of ammonia is:-
a. 3.6×10-5mol
L-1s-1
b. 1.2×10-5mol
L-1s-1
c. 2.7×10-5mol
L-1s-1
d. 1.8×10-5mol
L-1s-1
4. The
unit of rate constant of a first order reaction is:-
a. mol
L-1s-1
b. s-1
c. s-1(mol
L-1)-1
d. s-1mol2L-2
5. In
the rate law given by: rate =k[A][B], the overall order of the reaction is :-
a. 1
b. 0
c. 2
d. 3
6. For
a reaction when k = 2.5×103 L mol-1s-1, then
the order of the reaction is :-
a. 1
b. 2
c. 3
d. 0
7. The
half life in independent of initial concentration of reactants in :-
a. Zero
order reaction
b. First
order reaction
c. Second
order reaction
d. Third
order reaction
8. For
a first order reaction k = 2.5×10-4s-1, then the rate for
initial concentration of 0.01mol/L is :-
a. 2.5×10-4
mol/L/s
b. 2.5×10-3
mol/L/s
c. 2.5×10-6
mol/L/s
d. 2.1×103mol/L/s
9. For
a reaction
2N2O5→
4NO2 + O2
If the concentration of NO2
increases by 5.2×10-3M in 100s, then the rate of reaction is:-
a. 1.3×
10-5 M/s
b. 0.5×
10-5 M/s
c. 7.6×
10-4 M/s
d. 2.5×
10-5 M/s
10.
The half life of a first order reaction is
1min 40s. Calculate the rate constant.
a. 6.93×10-3
s
b. 6.93×10-3s-1
c. 4.95×10-3s
d. 1.73×10-3s-1
11.
In a reaction, A + B →
Product, rate is doubled when the concentration of B is doubled, and rate
increases by a factor of 8 when the concentrations of both the reactants (A and
B) are doubled, rate law for the reaction can be written as :-
a. Rate
= k[A] [B]
b. Rate
= k[A]2[B]
c. Rate
= k[A][B]2
d. Rate
= k[A]2[B]2
12.
The activation energy
for a reaction at the temperature T K was
found to be 2.303 RT J mol–1. The ratio of the rate constant to
Arrhenius factor is :-
a. 10–1
b. 10–2
c. 2
× 10–3
d. 2
× 10–2
13.For
a first order reaction (A) → products the concentration of A changes from 0.1M
to 0.025 M in 40minutes.The rate of reaction when the concentration of A is
0.01 M is:
a. 1.73
× 10–5 M/min
b. 3.47
× 10–4 M/min
c. 3.47
× 10–5 M/min
d. 1.73
× 10–4 M/min
14.
The rate of a chemical
reaction doubles for every 10°C rise of temperature. If the temperature is
raised by 50°C, the rate of the reaction increases by about
a.
64 times
b.
10 times
c.
24 times
d.
32 times
15.
The rate of reaction increases with temperature
due to
a. Decrease
in activation energy
b. Increase
in activation energy
c. Increase
in collision frequency
d. Increase
in concentration.
16.
The rate constant of a
first order reaction depends on
a. The
nature of the vessel
b. Initial
concentration of the reactant
c. The
temperature
d. The
time.
17.
The rate law for the reaction RCl + NaOH → ROH
+ NaCl is given by n = k[RCl]. Therefore
the rate of reaction will be
a. Independent
of the concentration of RCl
b. Doubled
on doubling the concentration of NaOH
c. Unaffected
by increasing the temperature.
d. Halved
when the concentration of RCl is halved.
18.
Rate constant for a reaction is 10-3
s-1. Calculate the time after which 25% of the reactants remain.
a. 693s
c. 6930s
d. 2029s
19.
For the reaction A + B → C, it is found that
doubling the concentration of A increases the rate by four times and doubling
the concentration of B doubles the reaction rate. What is the overall order of
reaction?
a. 4
b. 3/2
c. 3
d. 1
20.
The slope in Arrhenius plot is equal to
a. –Ea/2.303R
b. Ea/R
c. –R/2.303Ea
d. None
of the above.
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