The rate of the reaction 2NO + Cl 2 → 2NOCl is given by the rate equation rate = k[NO] 2 [Cl 2 ] The value of the rate constant can be increased by -

Increasing the concentration of NO.

Increasing the concentration of the Cl 2

Activation energy E a and rate constant (k 1 and k 2 ) of a chemical reaction at two different temperatures (T 1 and T 2 ) are related by -

l n k 2 k 1 = - E a R ( 1 T 2 - 1 T 1 )

I n k 2 k 1 = - E a R ( 1 T 2 + 1 T 1 )

I n k 2 k 1 = E a R ( 1 T 2 - 1 T 1 )

I n k 2 k 1 = - E a R ( 1 T 1 - 1 T 2 )

2 A → B + C ; It would be a zero order reaction when : -

The rate of reaction remains same at any concentration of A

The rate of reaction is proportional to square of concentration of A

The rate remains unchanged at any concentration of B and C

The rate of reaction doubles if concentraion of B is increased to double.

Chemistry - Chemical Kinetics - Quiz-10

Consider the reaction A $\to$ B. The concentration of both the reactants and the products varies exponentially with time. The figure that correctly describes the change in concentration of reactants and products with time is:

The graphs that represent a zero-order reaction are

(a)

(b)

(c)

(d)

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(a, b)
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(b, c)
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(c, d)
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(a, d)

The graphs that represent a first-order reaction are:

(a)

(b)

(c)

(d)

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(a, b)
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(b, c)
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(c, d)
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(a, d)

Match the graph given in Column I with the order of reaction given in Column II. More than one item in Column I may link to the same item of Column II :

Codes

i ii iii iv

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a b a b
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a b b a
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a a b b
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b b a a

Match the statements given in Column I and Column II :

Column I	Column II
A. Catalyst alters the rate of reaction	1. Proper orientation is not there always
B. $e^{- E_{a} / RT}$	2. By 'lowering the activation energy
C. Energetically favorable reactions are sometimes slow	3. Total probability is one
D. Area under the Maxwell-Boltzmann curve is constant	4. Refers to the fraction of molecules with energy equal to or greater than the activation energy

Codes
A B C D

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2 4 1 3
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3 1 4 2
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1 4 3 2
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3 4 1 2

Match the items of Column I and Column II :

Column I

Column II

A. Diamond

B. Instantaneous rate

C. Average rate

1. Short interval of time

2. Ordinarily rate of conversion is imperceptible

3. Long duration of time

Codes

A B C

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2 1 3
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1 2 3
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3 2 1
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1 3 2

Match the items of Column I and Column II :

Column I

Column II

A. Mathematical expression for the rate of reaction

B. Rate of reaction for zero-order reaction is equal to

C. Units of rate constant for zero-order reaction is same as that of

D. Order of a complex reaction is determined by

1. Rate constant

2. Rate law

3. Order of slowest step

4. Rate of reaction

Codes

A B C D

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3 4 1 2
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1 2 3 4
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2 1 4 3
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4 1 3 2

Assertion: The order of the reaction can be zero or fractional.

Reason: We cannot determine order from the balanced chemical equation.

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Both assertion and reason are correct and the reason is the correct explanation of assertion.
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Both assertion and reason are correct, but reason does not explain the assertion
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Assertion is correct, but the reason is incorrect.
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Both assertion and reason are incorrect.

Assertion: Order and molecularity are the same.

Reason: Order is determined experimentally and molecularity is the Sum of the stoichiometric coefficient of the rate-determining elementary step.

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Both assertion and reason are correct and the reason is the correct explanation of assertion.
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Both assertion and reason are correct, but reason does not explain the assertion
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Assertion is correct, but the reason is incorrect.
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The assertion is incorrect, but the reason is correct.

Assertion: Rate constant determined from the Arrhenius equation is fairly accurate for simple as well as complex molecules.

Reason: Reactant molecules undergo chemical change irrespective of their orientation during a collision.

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Both assertion and reason are correct and the reason is the correct explanation of assertion.
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Both assertion and reason are correct, but reason does not explain the assertion
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Assertion is correct, but the reason is incorrect.
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Both assertion and reason are incorrect.

The half-life for a zero order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in mol L^-1 s^-1) for the reaction is

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(1) $1.0 \times 10^{- 4}$
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(2) $2.0 \times 10^{- 4}$
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(3) $2.0 \times 10^{- 3}$
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(4) $1.0 \times 10^{- 2}$

In collision theory of chemical reaction, Z_AB represents

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the fraction of molecules with energies greater than E_a
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the collision frequency of reactants, A and B
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steric factor
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the fraction of molecules with energies equal to E_a

The unit of rate constant for a zero-order reaction is -

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$s^{- 1}$
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$mol L^{- 1} s^{- 1}$
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$L {mol}^{- 1} s^{- 1}$
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$L^{2} {mol}^{- 2} s^{- 1}$

The half life of a certain enzyme catalysed reaction is 138 s, that follow the 1st order kinetics.The time required for the concentration of the substance to fall from 1.28 mg L^–1 to 0.04 mg L^–1, is-

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276 s
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414 s
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552 s
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690 s

The rate of the reaction $2 N_{2} O_{5} \to 4 {NO}_{2} + O_{2}$ can be written in three ways:

$\frac{- d [N_{2} O_{5}]}{d t} = k [N_{2} O_{5}] \frac{d [N O_{2}]}{d t} = k' [N_{2} O_{5}] \frac{d [O_{2}]}{d t} = k'' [N_{2} O_{5}]$

The relationship between k and k′ and between
k and k′′ are-

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k′ = k, k′′= k
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k′= 2k; k′′= k
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k′= 2k, k′′= k/2
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k′ = 2k; k′′= 2k

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 -

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Increasing the concentration of NO.
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Increasing the concentration of the Cl₂
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Increasing the temperature
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All of the above.

Activation energy $E_{a}$ and rate constant (k₁ and k₂) of a chemical reaction at two different temperatures (T₁ and T₂) are related by -

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$l n \frac{k_{2}}{k_{1}} = - \frac{E_{a}}{R} (\frac{1}{T_{2}} - \frac{1}{T_{1}})$
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$I n \frac{k_{2}}{k_{1}} = - \frac{E_{a}}{R} (\frac{1}{T_{2}} + \frac{1}{T_{1}})$
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$I n \frac{k_{2}}{k_{1}} = \frac{E_{a}}{R} (\frac{1}{T_{2}} - \frac{1}{T_{1}})$
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$I n \frac{k_{2}}{k_{1}} = - \frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

A 300 gram radioactive sample has half life of 3 hour's. After 18 hour's remaining quantity will be :

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4.68 gram
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2.34 gram
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3.34 gram
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9.37 gram

The concentration of a solution is changed from 0.2 to 0.4, then what will be rate and rate constant. The reaction is of first order and rate constant is $K = 1 \times 10^{- 6}$ :

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$2 \times 10^{- 7}; 1 \times 10^{- 6}$
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$1 \times 10^{- 7}; 1 \times 10^{6}$
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$4 \times 10^{- 7}; 1 \times 10^{- 6}$
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$2 \times 10^{- 3}; 1 \times 10^{- 3}$

Half life of a radioactive sample is 4 days. After 16 days how much quantity of matter remain undecayed :

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$\frac{1}{4}$
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$\frac{1}{8}$
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$\frac{1}{16}$
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$\frac{1}{32}$

The rate of a first-order reaction is 1.5 ×10^–2 mol L^–1 min^–1 at 0.5 M concentration of the reactant. The half life of the reaction is:-

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23. 1min
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8.73 min
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7.53 min
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0.383 min

The bombardment of α-particle on $N_{7}^{14}$ emits proton then new atom will be :

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$O_{8}^{17}$
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$O_{8}^{16}$
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$C_{6}^{14}$
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Ne

Half life of a substance is 77 days then it's decay constant (days^-1) will be :

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0.9
0%
0.09
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0.009
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0.013

For the reaction $H^{+} + B r O_{3}^{-} + 3 B r^{-} \to 5 B r_{2} + H_{2} O$ the correct representation of the consumption & formation of reactants and products is :

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$\frac{d [B r^{-}]}{d t} = - \frac{3}{5} \frac{d [B r_{2}]}{d t}$
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$\frac{d [B r^{-}]}{d t} = \frac{3}{5} \frac{d [B r_{2}]}{d t}$
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$\frac{d [B r^{-}]}{d t} = - \frac{5}{3} \frac{d [B r_{2}]}{d t}$
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$\frac{d [B r^{-}]}{d t} = \frac{5}{3} \frac{d [B r_{2}]}{d t}$

₉₂U²³⁵, nucleus absorb a neutron and disintegrate in ₅₄Xe¹³⁹, ₃₈Sr⁹⁴ and x . The product x is : -

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3 - neutrons
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2 - neutrons
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α - particle
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β - particle

$3 A \to 2 B$ , rate of reaction $\frac{+ d [B]}{dt}$ is equal to :-

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$- \frac{3}{2} \frac{d [A]}{dt}$
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$- \frac{2}{3} \frac{d [A]}{dt}$
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$- \frac{1}{3} \frac{d [A]}{dt}$
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$+ 2 \frac{d [A]}{dt}$

$2 A \to B + C$ ; It would be a zero order reaction when : -

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The rate of reaction is proportional to square of concentration of A
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The rate of reaction remains same at any concentration of A
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The rate remains unchanged at any concentration of B and C
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The rate of reaction doubles if concentraion of B is increased to double.

For the reaction $2 N_{2} O_{5} \to 4 {NO}_{2} + O_{2}$ rate and rate constant are $1.02 \times 10^{- 4} and 3.4 \times 10^{- 5} \sec^{- 1}$ respectively, then the concentration of $N_{2} O_{5}$ at that time will be : -

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1.732 $m o l L -1$
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3.0 $m o l L -1$
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$1.02 \times 10^{- 4}$ $m o l L -1$
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$3.4 \times 10^{5}$ $m o l L -1$

When a biochemical reaction is carried out in a laboratory outside the human body in the absence of enzyme, then the rate of reaction obtained is $10^{- 6}$ times, then activation energy of reaction in the presence of enzyme is : -

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$\frac{6}{R T}$
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P is required.
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Different from, $E_{a}$ obtained in laboratory.
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Data is insufficient.

The activation energy for a simple chemical reaction A → B is E_a in forward direction. The activation energy for reverse reaction :

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Is negative of E_a
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Is always less than E_a
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Can be less than or more than E_a
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Is always double of E_a

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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