Question # 1

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

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

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

Born Haber cycle is used to determine the

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Lattice energy

Enthalpy of formation

Enthalpy of ionization

Enthalpy of dissociation

Spontaneous processes are mostly

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Reversible

Irreversible

Not irreversible

None of these

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 is not is state function

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Enthalpy

Entropy

Pressure

work

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

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

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

One of the following statements about Born-Haber cycle is correct. Which is that statement

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Born-Haber cycle is different from Hess's law

The energy change in a cyclic process is not zero

The lattice energy of the crystalline substances can be calculated easily

Heat of formation of the product and the lattice energy of the substance can be calculated simultaneously

For a given process, the heat chagnes of constant pressure and at constant volume are related to each other as.

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qp= qv

qp<qv

qp>qv

None of these

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

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

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

The optimum temperature for the synthesis of NH3 by Haber's process is.

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200 ^oC

300 ^oC

400 ^oC

500 ^oC

If an endothermic reaction is allowed to take place very rapidly i the air, the temperature fo the surrounding air.

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Remains constant

Increase

Decrease

Remain unchanged

In endothermic reactions, the heat content of the

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Products is more then that of reactants

Reactants is more than that of products

Both a and b

Reactant and products is equal

The sum of all kinds of energies of atoms, ions or molecules of a system is known as.

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Kinetic energy

Potential energy

Internal energy

Solar energy

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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

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

Which process is endothermic and spontaneous

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Neutralization of NaOH with HCl

Formation of NH3 from H2 and N2

Formation of H2O from H2 and O2

Evaporation of sea water

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

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