Question # 1

If a reaction involves only solids and liquids, which of the following is true?

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ΔH = ΔE

ΔΗ =ΔΕ

ΔH>ΔΕ

AH =AE +nRT

Neutralization of acid-base is

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Spontaneous

Exothermic

Non spontaneous

Both "a" and "c

If internal energy of the system is increased

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Change in state of the system may occur

Temperature of the system may rise

Chemical reaction may take place

All of these

By convention, the standard heat of formation of all elements is assumed to be

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Zero

positive

Negative

Infinity

What is not correct about ∆HF

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It is always negative

Ìts value gives an idea about the relative stability of reactants and the products.

Its value can be greater or less than zero

Value depends upon nature of bonds

Enthalpy of neutralization of strong acids and strong bases have same values because

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Neutralization leads to the formation of salt and water

Acids always give rise to H+ and bases always furnish OH-

Strong acids and bases are ionic substances

The net change involves the combination of H and OH ions to form water

Born-Haber cycle is an application of

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Hess's law

1" law of thermodynamics

Avogadro's law

1law of thermochemistry

One Joule is equivalent to

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4.184 cal.

0.4184cal.

1/2 cal.

1/4.184 cal

Which of the following processes has always. ∆H=-ve

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Formation of compound

Dilution of a solution

Dissolution of ionic compound

Combustion

According to Hess's law, the enthalpy change for a reaction

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Depends on path

Independent of the path

The sum of ∆E and ∆H

None of these

The enthalpy of formation of a compound is

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Positive

Either positive or negative

Negative

None

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