Question # 1

The study of which one of the followings guides to the mechanism of the reaction

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Order of reaction

Rate of reaction

Half-life period of reaction

Rate determining step

The order of reaction provides valuable information about of reaction

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Condition

Concentration

Mechanism

Parameters

Spectrometry method is applicable if a reactant or a product absorbs radiation

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Ultraviolet

Visible

Infrared

Any of these

Reaction kinetics is important to discover the---under which reaction will proceed most economically:

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rate constant

Conditions

volume

equilibrium point

In dilatometric method is directly proportional to extent of reaction

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Change in concentration

Change in pressure

Chang in volume

Change in temperature

By increasing the concentration of reactants, the rate of reaction

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Decreases

Increases

Remains constant

Not predicted

For reaction of methane and chlorine light is not available then

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Reaction will take place rapidly

No Reaction take place

Reaction occurs at double the rate

May all cases occur

Half-lives required to convert 100% reactant to produet for a first order reaction are

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10

1000

100

Infinity

If the reaction "P+Q→R+S' is deseribed as being of zero order with respect to P, it means that

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P is catalyst in this reaction

P molecules do not possess sufficient energy to react

The concentration of P does not change during the reaction

The rate of reaction is independent of the concentration of P

The increase in reaction rate as a result of increase in temperature from 10K to 90K is

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512

256

400

112

When does average rate become equal to instantaneous rate of reaction

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At the start of reaction

time interval is zero

at the end of reactior

time interval approaches zero

The slope of the graph is steepest at the beginning of reaction showing

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Rapid decrease in concentration of reactants

Rapid increase in concentration of reactants

Fast rate of reaction

All of the above

The number of reacting molecules whose concentration change during reaction is called

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Activated molecule

Rate of reaction

Order of reaction

half-life

The concentration of product is increasing from 30 mole/dm3 to 40mol/dm3 in 0.5 sec then rate of reaction will be------moledm-3sec-1

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0

20

15

25

The conversion of molecules of A to B follows a second order kineties. Doubling the concentration of A will inerease the rate of formation of B by a factor of

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2

4

1/2

1/4

The radioactive disintegration of 238U92 is

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First order

Second order

Third order

Zero order

In the reaction A+B→ Products, if B is taken in excess, then it is an example of

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Second order reaction

zero order reaction

Pseudo first order reaction

first order reaction

Which of the following reactions are usually slow?

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Neutralization of acids and bases

Displacement Reactions

Organic substitution reaction

Free radical reactions

The rate of reaction for a reaction is 30 mol dm-3sec-1 if the product of concentration of 10.reactant is unity the specific rate constant is

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25

2.5

30

15

The number of atoms or molecules whose concentrations determines the rate of a chemical reaction is called the

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Molecularity of the reaction

specific activity of the reaction

Order of the reaction

rate constant of the reaction

The reaction kinetics concerned with the

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Rate of reaction

Direction of reaction

Factor effecting rate of reaction

both a &b

Consider gas is measure in bars then the units of rate of reaction is

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Mole dm-3 sec

Bars sec

Mole dm-3 sec-1

Bars sec-1

Unit of the rate constant depends upon the

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Molecularity of reaction

Order of reaction

Concentration terms

Number of reactants

When the concentration of reactants is taken as unity the rate of reaction is equal to

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average rate

concentratian of reactant

instantaneous rate

specific rate constant

All the Hydrolytic reactions are

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First order

Second order

Third order

pseudo-first order

The rate of reaction between A and B increases by a factor of 100, when the concentration of A is increased 10 folds, the order of reaction with respect to A is

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10

1

4

2

The collision which results in chemical reaction

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Effective collision

Ineffective collision

Useless collision

All of the above

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