Question # 1

The net heat change in a chemical reaction is same whether it is brought about in two or more different ways in one or several steps. It is knnown as

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Henry's law

Hess's law

Joule's principle

Law of combustion

If an endothermic reaction is allowed to take place very rapidly in the air, the temperature of the surrounding air

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Remains constant

Increase

Decrease

Increase a bit

The S.I. units for the molar heat capacity are

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Joule Cm^-3degree^-1

Joule deg^-1atm^-1

Joule deg^-1mol^-1

Joule deg^-1kg^-1

Born Haber cycle is used to determine the

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Lattice energy

Enthalpy of formation

Enthalpy of ionization

Enthalpy of dissociation

Which one of the following enthalpies is always an exothermic process.

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Enthalpy of atomization

Enthalpy of neutralization

Enthalpy of ionization

Enthalpy of dissociation

Standard enthalpy change when one mole of compound is formed from their elements at standard state is.

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Heat of formation

Standard heat of formation

Heat of combustion

Standard Heat of neutralization

Spontaneous processes are mostly

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Reversible

Irreversible

Not irreversible

None of these

the value of delta H and delta E for liquids and solids is almost same because.

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No change in temperature

Heat absorbed

No change in volume

Heat evolved

Which is not is state function

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Enthalpy

Entropy

Pressure

work

The net change in a chemical reaction is same whether it takes place directly or indirectly is

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Henry's law

Charles's

Hess's lass

Graham's law

The pressure of oxygen inside the bomb calorimeter is.

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100 atm

50 atm

25 atm

20 atm

Which of the following statement is contrary to the first law of thermodynamics

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An equivalent amount of heart energy can neither be created nor destroyed

One form of energy can be transferred into an equivalent amount of other kinds of energy

In an adiabatic process, the work done is independent of its path

Continuous production of mechanical work without supplying an equivalent is amount of heat possible

The change in heat energy of a chemical reaction at constant temperature and pressure is called

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Enthalpy change

Bond energy

Heat of sublimation

Internal energy change

Which of the following value of heat of formation indicates that the product is least stable.

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-94 KJ

-231.6 KJ

+21.4 KJ

+70 KJ

Most of the reaction which give stable products are

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Exothermic

Endothermic

Isothermal

None of these

Whenever a reaction is endothermic, then it means that

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Heat is transferred from surrounding to the system

Heat is transferred system to the surrounding

Heat content of the product is greater than that of reactants

Heat content of the reactants is greater than the products

In endothermic reactions, the heat content of the.

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Products is more than that of reactants.

Reactants is more than that of products

Both a and b

Reactants and products are equal

A material or a collection of materials which is under study is called

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State function

Degree and joule

Degree and ergs

Calorie and joule

The enthalpy of combustion is

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Positive

Negative

Either positive or negative

No correlation

What happens to the enthalpy change when the coeffficients of a chemical equation are douubled

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It doubles

It becomes half

It does not change

It cannot be predicted

Which substance have delta E = Delta H and no pressure - volume work.

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Liquids only

Solids only

Gases only

Liquids and solids

The net heat change in a chemical reaction is same whether it is brought about in two or more different ways in one or several steps. It is known as

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Henry's law

Hess's law

Joule's principle

Law of conservation of energy

At constant volume of a system remains constant and the heat is absorbed by the system, them amount of heat absorbed is called

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Enthaply change of the system

Internal energy change of the system

Total enthalphy of the system

Total internal energy of the system

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Heat of reaction

Heat of sublimation

Heat of neutralization

Heat of combustion

A chemical change always involve

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Absorption of heat

Evolution of heat

Either absorption or evolution of heat

The liberation of heat and light energy

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