MDCAT CHEMISTRY-Reaction Kinetics (SMART INSTITUTE)

A visually appealing image representing chemical reactions and reaction kinetics, featuring lab equipment like beakers, molecules, and activation energy diagrams.

MDCAT Chemistry: Reaction Kinetics Quiz

Welcome to the MDCAT Chemistry quiz focused on Reaction Kinetics! This quiz tests your understanding of key concepts and principles related to chemical reactions and their rates.

Prepare yourself to explore:

Activation Energy
Order of Reactions
Catalysis and its characteristics
Half-life calculations

60 Questions15 MinutesCreated by CalculatingAtom42

01-Activation energy of a reaction

Includes the averrage kinetic energy of the reactants

Is in addition to the average K.E of the reactants

Is in addition to the average K.E of the products

Required for effective collision

02-Ea appears as a potential energy hill between .... .for carrying out the reaction.

A) among the reactants

Reactants and products

Among the products

None of above

03-Slope of the graph between 1/T and log k gives

A) reaction rate

B) activation energy

C) specific rate constant

Both b and c

04-The unit of rate constant is the same as that of the rate of reaction in

1st order reaction

Zero order reaction

2nd order reaction

3rd order reaction

05-Arrhenius equation can be used for evaluating

A) specific rate constant

B) half life period

C) activation energy

Both a and c

06-A catalyst can

Accelerate the reaction rate

Retard the reaction rate

Chemically un-consumed at the end of the reaction

All of above

07-The 2nd order reaction becomes 1st order when

One of the reactants is limiting

One of the reactants is in large excess

None of the reactants is in large excess

Both reactants in large excess

08-Oxidation of SO2 (g) in the presence of NO (g) catalyst is an example of

Homogeneous catalysis

Heterogeneous catalysis

Auto catalysis

Negative catalysis

09-Oxidation of SO2 (g) in the presence of V2O5 (s) is an example of

Homogeneous catalysis

Heterogeneous catalysis

Auto catalysis

Negative catalysis

10-WOF is not a characteristic of a catalyst

It is specific in its action

Provide the reactants a low activation energy barrier

Becomes chemically changed at the end of a reaction

It can be poisoned by an impurity which deactivates its catalytic capability

11-The specific constant of a chemical reaction is the rate of the reaction when the concentration of the reactant is

Less than unity

Greater than unity

Equal to unity

Equal to the concentration of 2nd order reaction

12-The half-life time for a 1st order decomposition of a substance dissolved in CCl4 is 2.5 hours at 30 'C. The amount of substance left after 10 hours if the initial weight of the substance is 160 g

15 g

10g

20g

13-An endothermic reaction A → B has an activation energy 15 kcal / mol and the heat of the reaction 5 kcal/mol. The activation energy for the reaction B → A will be

20 kcal / mol

10 kcal / mol

15 kcal / mol

None of above

14-The rate of reaction is doubled for every 10 'C rise in temperature. The increase in reaction rate as a result of temperature rise from 10 'C to 100'C is:

112

400

512

614

15-For the 1st order decomposition reaction 2N2O5 (g) → 4NO2 (g) + O2(g) ,the half-life is given as:

0.693 / k

Log2 / k

0.693 / 2k

In2 / k

16-WOF is correct about following reaction if iron is not 100 % pure? 2Fe + 3H2O → Fe2O3.3H2O

Very fast reaction

Moderately slow reaction

Very slow reaction

Not predicted

17-For a chemical reaction to occur

The vessel shall be open

Reacting molecules should have less energy than at time of collision

Reacting molecules must be properly oriented and energy more than or equal to Ea

The reacting molecules must not collide with each other

18-The reaction that involves gases, its rate does not depend upon

Catalyst

Partial pressure

Temperature

Concentration

19-The mathematical relation between the rate of reaction and the concentration s of the reactants is known as the

Rate equation

Arrhenius equation

Rate law

Rate law and rate equation

20-Which one affects the specific rate constant

Temperature

Concentration of reactants

Catalyst

All of these

21-When the concentration of reactant in the reaction is increased by 8 times, the rate increased by 2 times. The order of reaction is

1/2

1/3

22-If 75 % of any given amount of radioactive element disintegrates in 60 min. The half-life of radioactive element is:

20 min

30 min

45 min

25 min

23-The unit of rate constant of second order reaction is

Mol dm-3 sec-1

Mol-2 dm+6

Sec-1

Mol-1 dm+3 sec-1

25-If the energy of the activated complex lies close to energy of reactants, it means that reaction is:

Slow

Endothermic

Exothermic

Exothermic and fast

26-WOF statements regarding a catalyst is not true.

A catalyst does not alter the equilibrium in a reversible reaction

A catalyst can initiate the reaction which is not thermodynamically favourable

Catalytic reactions are very specific in nature

A catalyst remains unchanged in composition and quantity

27-Radiations are absorbed in

Spectro photometer reaction

Optical rotation method

Dilatometric method

Refractrometric method

28-Hydrolysis of ethyl acetate into acetic acid and ethanol in the presence of mineral acid

Fractional order reaction

1st order reaction

Pseudo 1st order reaction

2nd order reaction

29-When potential energy of the transition state is very high, then WOF results is applicable?

Low activation energy and fast reaction

High activation energy and fast reaction

Low activation energy and slow reaction

High activation energy and slow reaction

30-The energy of activation complex is

A) less than reactants

B) greater than products

C) greater than reactants

Both b and c

31-The activation energy for a simple chemical reaction A → B is Ea in forward direction. The activation energy for reverse reaction

Can be less than or more than Ea

Is negative of Ea

Is always double of Ea

Is always less than Ea

32-For a reaction A + 2B → C , rate is given by +d[C] / dt = k [A] [B], hence the order of the reaction is

33-The rate of reaction depends upon

Molar concentration

Equivalent mass

Atomic mass

None of these

34-For a first order reaction, the half-life period is independent of

Initial concentration

First power of final concentration

Cube root of initial concentration

Square root of final concentration

35-Activation energy of a chemical reaction can be determined by

Evaluating rate constant at standard temperature

Evaluating velocities of reaction at two different temperature

Evaluating rate constants at two different temperature

Changing concentration of reactants

37-WOF best explains the effects of a catalyst on the rate of a reversible reaction?

It decreases the rate of the reverse reaction

It increases the kinetic energy of the reacting molecules

It moves the equilibrium position to the right

It provides a new reaction path with a lower activation energy

38-For a chemical reaction A → B, the rate of reaction doubles when the concentration of A is increased four times. The order of reaction for A is

Zero

Two

One

Half

39-Among the following is incorrect about order of reaction

It is calculated experimentally

It is sum of powers of concentration in rate law expression

The order of reaction cannot be fractional

There is not necessarily a connection between order and stoichiometry of a reaction

40-Among the following factors, the specific reaction rate of a first order reaction depends upon

Temperature

Pressure

Concentration of reactants

Volume

41-The rate of reaction is defined as

Decrease in the concentration of a reactant

Increase in the concentration of a product

Change in concentration of any one of the reactant or product per unit time

All of these

42-For the reaction A + B + C → Product, Rate = K[A]^1/2 [B]^1/3 [C]. The order of reaction is

6/6

11/6

43-The dimension of the rate constant of a third order reaction involves:

Only time

Time and square of concentration

Time and concentration

Only concentration

44-In the reaction A + B → Product. The doubling of [A] increases the reaction rate four times but the doubling of B has no effect on rate. The expression is

Rate = K [A]^2

Rate = K [A]^2 [B]^2

Rate = K [A]

Rate = K [A] [B]

45-The equation for the rate constant is k=A^-Ea/RT A. Chemical reaction will proceed more rapidly if there is a decrease in

46-For a chemical reaction, which can never be a fractional number

Oredr

Molecularity

Half-life

Rate constant

47-WOF is a reaction of zero order?

H2 +Cl2 → 2HCl (hv)

2HI → H2 + I2

2N2O5 → 4NO2 + O2

H2 + Br2 → 2HBr

48-A catalyst is a substance which

Supplies energy to the reaction

Increases the equilibrium constant of the reaction

Changes the equilibrium constaant of the reaction

Shortens the time to reach equilibrium

49-A reaction involving two different reactants can never be a

Bimolecular reaction

First order reaction

Uni-molecular reaction

Second order reaction

50-When concentration of reactants is increased eight times the rate becomes two times, the order of reaction is

1/3

1/2

1/4

51-The rate determining step in a reaction is A + 2B → C. Doubling the concentration of B would make the reaction rate

Two times

Four times

Same rate

1/4 times

52-The rate law of a reaction is Rate = k [A]^2 [B]. On doubling the concentration of both A and B, the rate X will become

X^3

4X^2

53-For the reaction CH3COCH3 + I2 + H+ → Product. The rate is governed by Rate = k[CH3COCH3] [H+] the rate order of I2 is

54- 2A + 2B → D + E for the reaction following the mechanism has been proposed 1. A + 2B → 2C + D (slow) 2. A + 2C → E (fast)

Rate = k [A]^2 [B]^2

Rate = k [A] [B]^2

Rate = k [A]^2 [B]^2 [C]

Rate = k [A] [B]

55-For a reaction 2A + B → Products, Reaction Rate = K [A][B]^2 . Concentration of A is doubled and that of the B is halved, the rate of reaction will be

Doubled

Unaffected

Halved

Four times

56-In a reaction, concentration of reactant A is increased by 16 times, the rate increased only two times, the order of the reaction would be

1/2

1/4

57-In the reaction A → B when the concentration of A is changed from 0.1 M to 10 M, the rate of reaction increases by a factor of 100. The order of reaction w.r.t A is:

58-For the reaction A + B → C + D, doubling the concentration of both the reactions increases the reaction rate by 8 times and doubling the initial concentration of B simply doubles the reaction rate. The rate law for the reaction is

Rate = k [A] [B]^2

Rate = k [A]^1/2 [B] ^2

Rate = k [A] [B]

Rate = k [A]^2 [B]

59-The rate constant of a reaction has same units as the rate of reaction. The reaction is

3rd order

1st order

2nd order

0th order

MDCAT CHEMISTRY-Reaction Kinetics (SMART INSTITUTE)

MDCAT Chemistry: Reaction Kinetics Quiz

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