Chemical kinetics

Question 1

Feasibility of a chemical reaction can be predicted by

Answer 1

Thermodynamics

Question 2

Extent of a chemical reaction can be predicted by

Answer 2

Chemical equilibrium

Question 3

Assertion : diamond cannot be converted to graphite
Reason : diamond is forever

Answer 3

The assertion and reason is false diamond can be converted to graphite

Question 4

The rate is always multiplied with -1 to make it a positive quantity

Answer 4

True

Question 5

Unit of rate is

Answer 5

Concentration time inverse/ atm s inverse

Question 6

Statement 1: Rate of a reaction depends on stochiometric coefficient
Statement 2: rate of any species will be fixed value under given condition

Answer 6

Both statements are correct

Question 7

The rate of the reaction is CHCL3 +CL2 = CCL4 + HCL

Answer 7

Rate = k [ CHCl3] [ Cl2]^1/2

Question 8

The rate ofthe reaction is CH3COOC2H5 + H2O = CH3COOH + C2H5OH

Answer 8

Rate = k[ CH3COOC2H5] ^1 [H20]^0

Question 9

Assertion: rate law of a reaction cannot be determined by mere looking of a chemical reaction
Reason : it must be obtained experimentally

Answer 9

Both assertion and reason are true

Question 10

Example of consecutive reaction is

Answer 10

Oxidation of ethane

Question 11

Example of reverse reaction and side reaction

Answer 11

Nitration of phenol to yield o nitro phenol and p nitro phenol

Question 12

Statement1: the reaction with collision of three or more molecules are rare to proceed
Statement2 : 2NO +O2 = 2NO2

Answer 12

Both statements are correct

Question 13

The order of the given reaction is KCLO3 + 6FeSO4 +3 H2SO4 = KCL +3 Fe2(SO4)3 +3H20

Answer 13

2

Question 14

In Decomposition of hydrogen peroxide the rate determining step is

Answer 14

H2O2 + I^- = H2O + IO ^-

Question 15

Statement1: order is applicable to elementary as well as complex Rn but
Statement2 : molecularity is applicable only to elementary rn

Answer 15

Both statements are true

Question 16

Factors influencing the rate of the reaction is

Answer 16

Concentration of reactant
Rate expression and rate constant
Order of a reaction
Molecularity of a reaction

Question 17

The integrated rate eq for 1st order rn
Is

Answer 17

[R] = -KT +[ Ro]

Question 18

Statement 1: some enzyme catalyzed rn and reaction which occur on the metal surface are examples of zero order rn
Statement2: zero order reactions are very rare

Answer 18

Both statements are true

Question 19

Why is 2 NH3 = N2 + 3H2 (in presence of Pt catalyst and 1130 K) a zero order rn ?

Answer 19

This reaction is catalyzed by Pt , at high pressure the metal surface is saturated with gas molecules and further changes in reaction condition cannot alter the amountt of ammonia making the rate of reaction concentration independent

Question 20

Examples of zero order rn

Answer 20

NH3 = N2 + H2 ( in presence of Pt and at 1130K)
Thermal Decomposition of HI on gold surface

Question 21

The integrated form of 1st order reactions are

Answer 21

[R] = [Ro] e ^ (-kt)
K = 2.303 /t log [ Ro]/ [ R]

Question 22

Examples of first order reaction

Answer 22

Hydrogenation of ethene
All artificial and natural radioactive decay of unstable nuclei
Decomposition of N2O5 and N2O

Question 23

For zero order reaction half life is

Answer 23

[Ro] /2 k

Question 24

For first order reaction half life is

Answer 24

0.693 / k

Question 25

Statement 1: straight line plot of zero order rn Is btw [ R] vs t
Statement 2: straight line plot of 1st order rn Is btw ln[ R] vs t

Answer 25

Both statement are correct

Question 26

Order of a reaction can be altered by conditions

Answer 26

True

Question 27

Examples of pseudo first order rn Is

Answer 27

Inversion of cane sugar
Hydrolysis of ethyl acetate in presenceof Excess water

Question 28

For a chemical reaction the rate constant is doubled for every

Answer 28

10° rise in temp

Question 29

The temp dependence of a chemical reaction is explained by arrhenius eq

Answer 29

K = Ae ^ (- Ea / RT) where A is arrhenius factor or frequency factor

Question 30

Activation energy is measured in

Answer 30

Joules per mole

Question 31

Statement 1 : all molecules of reacting species have same kinetic energy
Statement 2 : that is why Ludwig boltzmann and James Clark maxwell used to statistics to predict the behavior of large number of molecules

Answer 31

Statement 1 is incorrect while statement 2 I correct

Question 32

Increasingthe temp increases the fraction of molecules which collide with more than Ea

Answer 32

True

Question 33

Arrhenius eq in log form is

Answer 33

Log k2/ k1 = Ea /2.303 R [ T2- T1/ T1T2]

Question 34

Explain the action of catalyst

Answer 34

The catalyst take part in chemical reaction by forming temporary bonds with the rectant which form an intermediate complex which has transitory existence and Decomposes to yield products

Question 35

Assertion : catalyst does not alter Gibbs energy
Reason : it does not catalyse non Spontaneous rn

Answer 35

Both assertion and reason are true but it’s not the reson of assertion

Question 36

Collision theory is based on

Answer 36

Kinetic theory of gases

Question 37

Define Collision frequency

Answer 37

It is number of collision per sec per unit volume of a reaction mixture

Question 38

Rate according to collision theory

Answer 38

Rate =P Z e^(- Ea/RT) where p is probability factor or steric factor