Question # 1

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Zero

1

2

1.5

The sum of the exponents of the conc. terms in the rate equation is called

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Rate of reaction

Order of reaction

Specific rate constant

Average rate

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Rate = k[FeCl₃] [Kl]²

Rate = k[Fe⁺³][Cl^-1] [Kl]

Rate = k[Fe⁺³] [Cl^-1][K;]

Rate = k[Kl]³[FeCl₃]°

Optical rotation method is sued when

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Reaction involve ions

Change of refractive indices

Reactions involving change of optical activity

None of the above

Which of the following may affect the rate constant (k) fro a reaction :

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Change in concentration.

Change in pressure.

Change in pH.

Change in temperature.

The unit of rate of reaction is

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mole dm^-3

mole Kg^-1

moles dm^-3sec^-1

grams dm^-3

When we perform the same reaction by taking two different initial concentrations of a reactant for a second order reaction then

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Reaction becomes exothermic

Energy of activation is different

Mechanism of reaction is changed

Half life period is changed

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

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Third order reaction

Second order reaction

First order reaction

Zero order reaction

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Small change in concentration of product

Small time internal

Co-efficient of the reactant

Co-efficient of the product

The factor which effect the rate of reaction

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Nature of reactants

Surface area

Light

All of the above

By the use of catalysis the energy of activation is

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Decreased

Increased

Not affected

None

The actual number of atoms or molecules taking part in rate determining step is

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Rate of reaction

Velocity of reaction

Order of reaction

Molecularly

which one of the following is a heteroheneous catalysis

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When copper is allowed to react with HNO₃, the reaction is slow in the beginning, finally becomes very fast. It is due to the formation of an auto catalyst which is

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Cu(NO₃)₂

CuO

O₂

HNO₂

Group l-A elements react with water fastly than the reaction of group ll-A elements because

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l_Aelements are more soft then ll_A

l_Aelements are non-metals

l_Aelements have 1 electron in their outermost s-orbital and are strongly electropositive

l_Aelements make ionic bond

Hydrogenation of vegetable oils is accelerated by Ni catalyst. The catalytic activity of Bi is increased by a promoter of activator which is

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Na and K

Na and Hg

Hg and Zn

Cu and Te

Complex protein molecules which catalyses the organic reactions in the living cells are called

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Living organisms

Enzymes

Viruses

Bacteria

When initial concentration of reactants an order of reaction is given, then its half life period can be calculated by the equation

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Which statement about Arrhenius equation is incorrect

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Factor 'A' called Arrhenius constant depends upon collision frequency of reactants

Rate of reaction increase by increasing temperature

Rate constant k is increased

Activation energy Ea is decreased by rise in temperature

If the rate equation of a reaction 2A+B-------->Products is , Rate = K[A] [B], and A is present in large excess, then order of reaction is :

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1

2

3

Above

The rate constant k of a reaction activation energy Ea and temperature are related by Arrhenius in the form of an equation which is

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Which technique is used to determine the absorption of radiations?

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Dilatometer method

Optical rotation method

Spectrometry

Refractometric method

Half life period of N₂O₅is 24 minutes and it remains same where we increase or decrease its initial concentration, then reactions

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Zero order

First order

Second order

Third order

In the hydrolysis of CH₃COOC₂H₅the acid produced is

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Inhibitor

Catalyst

Auto catalyst

None of above

All reactions occur in :

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A single step.

A series of steps

Two steps.

Both (a) and (b)

The rate of reaction is denoted by

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dc/dp

dc/ac

dc/dT

dc/dt

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Rate is independent of concentration of water since it is in excess

Rate is independent of concentration of ester since it is in exces

Rate depends upon the concentration of acid catalyst added

Rate = k[CH₃COOC₂H₅]^1/2[H₂O]^1/2

The rate of reaction between two specific time intervals is called

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Instantaneous rate

Average rate

Specific rate

Ordinary rate

In exothermic reaction decrease in potential energy of the products will result in

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Decreases in kinetic energy of the particles

Increases in kinetic energy of the particles

No change in kinetic energy

Decreases in activation energy

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1st order

2nd order

Zero order

3rd order

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Initial concentration of reaction

Initial concentration of products

Final concentration of products

Order of the reaction

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