Question # 1

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

Calorie is equivalent to

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0.4184J

4.184J

418.4J

40.18J

What is correct about heat of combustion

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It is applicable to gaseous substances only

It is always negative

It is always positive

It is positive in some cases while negative in other

The heat of reaction depends upon

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Temperature of the reactants

Physical states of the reactants and the products

Both A) and B)

Path of the reaction and the temperature

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

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

How much heat is absorbed by 100 g of water when its temperature decreases from 25°C to 5°C? (heat capacity is 4.2 J/gK)

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84,000J

2000/4.2J

-2000/4.2j

-8400J

Total heat content of a system is called

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Internal energy

Entropy

Enthalpy

All of these

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

During an exothermic or endothermic reaction which one of the following formula is used to calculate the amount of heat evolved or absorbed

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ΔΗ = ΔΕ+PV

∆E= q+w

Δp =ΔΗ

q = m x s x ∆T

The lattice energy of NaCl is

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787 j/ mole

790 kj/mol

780 kJ/ mol

-787 kI / mole

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