Question # 1

In which of the following techniques rate of reaction is directly related with number ofions

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Spectrometry

Dilatometric method

Conductometric method

Refractometric method

Substance which is formed as well as consumed during a chemical reaction and have temporary existence.

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Reactant

product

Catalyst

Intermediate

If the rate of the reaction is equal to the rate constant, the order of the reaction is

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3

1

0

2

Amount of product formed increases with time, this statement is true for reactions-------with kinetics

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1s order

3rd order

zero order

Any order

If reactants are conductor of electricity, then method is used to measure the change in concentration of reaction

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Optical rotation

Refractrometric

Dilatometric

Electrical conductivity

The reaction which is zero order

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Decomposition ofN2O5

Formation of Glucose in plant

Formation of Fel2

Chorination of methane in sunlight

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

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

Rusting of iron is the example of

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Fast

Slow

moderate

depends upon conditions

Rate of which reaction increases with temperature?

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Exothermic and endothermic reactions

Endothermic reactions

Exothermic reactions

None of these

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 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 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

Higher the surface area available for reaction

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slower the reaction

faster the reaction

constant the reaction

lower the Ea

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

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

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

For a chemical reaction in which one of the reactant also act as solvent, the order will be

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First order

Third order

Second order

pseudo-first order

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

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

All the Hydrolytic reactions are

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First order

Second order

Third order

pseudo-first order

Doubling the pressure in a liquid phase reaction

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Will double the rex

Will increase the rex

Will decrease the rex

Will not alter the concentration of reactant

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

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

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

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10

1000

100

Infinity

The collision which results in chemical reaction

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Effective collision

Ineffective collision

Useless collision

All of the above

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

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