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12th Chemistry weekly Test - 4 (Chemical Kinetics )

St. Britto Hr. Sec. School - Madurai

12th Chemistry weekly Test - 4 (Chemical Kinetics )-Aug 2020

Time : 1.00 Hours

Part - A

Multiple Choice Question - Answer All Question

Enzymes increase the rate of reactions.

By lowering activation energy
By increasing activation energy
By changing equilibrium constant
By forming enzyme substrate complex

What would be the rate of disappearance of oxygen, if the rate of formation of nitric oxide (NO) is 3.6 xl0^-3mol L^-1 s^-1?

4 x10^-3mol L^-1s^-1
4 x10^-3mol^-1 L^-1s^-1
4.5 x 10^-3mol L^-1s^-1
4.5 x 10^-3mol^-1 L^-1s^-1

Activation energy of a reactant is reduced by ___________________

increased temperature
reduced temperature
increased pressure
reduced pressure

In a first order reaction \(x\longrightarrow y\) if k is the rate constant and the initial concentration of the reactant x is 0.1M, then, the half life is

\(\left( \cfrac { log2 }{ k } \right) \)
\(\left( \cfrac { 0.693 }{ (0.1)k } \right) \)
\(\left( \cfrac { In2 }{ k } \right) \)
none of these

The excess energy which a molecule must possess to become active is known as

kinetic energy
threshold energy
potential energy
activation energy

The rate of a reaction is expressed as k[A]₂[B]¹, the reaction is said to be

second order with respect to A
first order with respect to B
overall order of the reaction is third order
all the above

Pick out the odd one.

₉₂U²³⁸ ⟶ ₉₀Th²³⁴ + ₂He⁴
SO₂ Cl₂ ⟶ SO₂ + Cl₂
CH₃ COOCH₃ + H₂O \(\overset { { H }^{ + } }{ \longrightarrow } \) CH₃ COOH + CH₃ OH
C₁₂ H₂₂ O₁₁ + H₂O \(\overset { { H }^{ + } }{ \longrightarrow } \) C₆ H₁₂ O₆ + C₆ H₁₂ O₆

What would be the activation energy of a reaction when the temperature is increased from 27^oC to 37^oC?

534 kJ mol^-1
53.4 kJ mol^-1
5.34 kJ mol^-1
None of these

The magnitude of order of a reaction may be _____________

fractional
zero
integral values
all of these

By the order of reaction we mean _______________

the sum of powers to which the concentration terms are raised in the rate equation
the number of reactants take part in the reaction
the number of concentration terms in the velocity equation for the reaction
the least number of product molecule needed for the reaction

A reaction having equal activation energies for forward and reverse reactions has

ΔG = 0
ΔH = 0
ΔH = ΔG = ΔS = 0
ΔS = 0

How much time will be taken for 20 gm to reduce 5 g? [R = 2 x 10^-3s^-1 (I order reaction)]

693.1 s
693.1 s^-1
6.931 s
6.931 s^-1

All radioactive transformations follow________ order kinetics.

zero
first
second
third

For the reaction \({ N }_{ 2 }{ O }_{ 5 }\left( g \right) \longrightarrow { 2NO }_{ 2 }\left( g \right) +\cfrac { 1 }{ 2 } { O }_{ 2 }\left( g \right) \) value of rate of disappearance of N₂O₅is given as 6.5X10-² molL^-1s^-1 The rate of formation of NO₂ and O₂ is given respectively as

(3.25X10^-2 mol L^-1S^-1) and (1.3 X 10^-2 mol L^-1s^-1)
(1.3X10^-2 mol L^-1s^-1) and (3.25 X10^-2 mol L^-1s^-1)
(1.3X10^-1mol L^-1s^-1) and (3.25 X10-2 mol L^-1s^-1)
None of these

2A ⟶ B + C. It would be a zero order reaction when

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

The half-life period of a first order reaction is 69.3 seconds. Its rate constant is _______________.

10^-2 s^-1
10^-4 s^-1
10 s^-1
10² s^-1

2N₂O₅ ⟶ NO₂ + O₂, \(\frac { d\left[ { N }_{ 2 }{ O }_{ 5 } \right] }{ dt } \) = k₁[N₂O₅], \(\frac { d\left[ { NO }_{ 2 } \right] }{ dt } \)= k₂[N₂O₅] and \(\frac { d{ O }_{ 2 } }{ dt } \) = k ₃[N₂O₅], the relation between k₁, k₂ and k₃ is

2k₁ = 4k₂ = k₃
k₁ = k₂= k₃
2k₁ = k₂ = 4k₃
2k₁ = k₂ = k₃

The addition of a catalyst during a chemical reaction alters which of the following quantities? (NEET)

Enthalpy
Activation energy
Entropy
Internal energy

A zero order reaction X ⟶ XProduct, with an initial concentration 0.02M has a half life of 10 min. if one starts with concentration 0.04M, then the half life is

10 s
5 min
20 min
cannot be predicted using the given information

When the E_a of a reaction zero then the rate constant of the reaction is equal to __________

2.303 K
\(\frac { K }{ 2.303 } \)
\(\left( { t }_{ \frac { 1 }{ 2 } } \right) \)
A

In any unimolecular reaction _______________

Only two reacting species is involved in the rate determining step.
The order and the molecularity of slowest step are equal to one.
The molecularity of the reaction is one and order is zero.
Both molecularity and order of the reaction are one.

CH₃COOCH₃ + H₂O \(\overset { { H }^{ + } }{ \longrightarrow } \) CH₃COOH + CH₃OH is an example of _______ order reaction.

first
zero
third
pseudo

In a reversible reaction, the enthalpy change and the activation energy in the forward direction are respectively −x kJ mo^l-4 and kJ mol^-1 Therefore , the energy of activation in the backward direction is

(y-x)kJ mol-¹
(x+y)J mol^-1
(x-y)KJ mol^-1
(x+y)X10³Jmol^-1

In the graph showing Maxwell, Boltzmann distribution of energy _______________

area under the curve must not change with increase in temperature.
area under the curve increases in temperature.
area under the curve decreases with increase in temperature.
None of these above

Rate law cannot be determined from balanced chemical equation if _____________

Reverse reactions is not involved
It is an elementary reaction
It is a sequence of elementary reactions
All of the reactants is in excess. Rate law can be determined from balanced chemical equation if it is an elementary reaction.

Compound A reacts by first order kineties. At 25^oC, the rate constant of the reaction is 0.60 see:'. What is the half life of A?

1.15 sec
0.4158 sec
0.093 sec
1.29 sec

For a first order reaction A u27f6 product with initial concentration x mol L^-1, has a half life period of 2.5 hours. For the same reaction with initial concentration \(\left( \frac { x }{ 2 } \right) \) mol L-1 the half life is

(2.5 x 2) hours
\(\left( \frac { 2.5 }{ 2 } \right) \)hours
2.5 hours
Without knowing the rate constant, t_1/2 cannot be determined from the given data

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200K to 400K? (R = 8.314 JK-1mol^-1)

234.65 kJ mol^-1 K^-1
434.65 kJ mol^-1 K^-1
434.65 J mol^-1 K^-1
334.65 J mol^-1 K^-1

The rate constant of a first order reaction is 2.0 x 10^-6 s^-1. The initial concentration of the reactant is 0.10 mol dm^-3. What is the I value of the initial rate?

2.0 x 10^-7 mol dm^-3 s^-1
2.0 x 10^-6 mol dm^-3 s^-1
2.0 x 10^-5 mol dm^-3 s^-1
2.0 x 10⁷ mol dm^-3 s^-1

The addition of a catalyst during a chemical reaction alters which of the following quantities?

Activation energy
Entropy
Internal energy
Enthalpy

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