Question # 1

The value of ∆V being very small. The term P∆V can be neglected for process involving

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Liquid and gas

Solids and gases

Liquid and solid

None of these

One of the best applications of Hess's law to calculate the lattice energy of ionic compound is

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Measurement of enthalpy change in a calorimeter

Studying of first law of thermodynamics

Measurement of a heat of formation of a compound

Born-Haber cycle

One Joule is equivalent to

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4.184 cal.

0.4184cal.

1/2 cal.

1/4.184 cal

Decomposition of H2O is

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Endothermic reaction

Nuclear reaction

Exothermic reaction

Zero nuclear reaction

Whenever a reaction is endothermic, then it means that

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Heat is transferred system to the surrounding

Heat is transferred from surrounding to the system

Heat content of the products is less than that of reactants

Heat content of the reactants is greater than the products

Calorie is equivalent to

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0.4184J

4.184J

418.4J

40.18J

One kilo calorie is equal to

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4.184J

1000J

4184J

1kJ

Enthalpy of a reaction can be measured by

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Glass calorimeter

Barometer

Manometer

Thermometer

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 measurement of enthalpy change at standard conditions means that we should manage the measurement at

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24°C at 1 atm

25°C at 1 atm

0C° at 1 atm

100C° 1 atm

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

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Zero

positive

Negative

Infinity

ΔH° represent the enthalpy change at

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0°C and 1 atm pressure

25°Cand 1atm

0K and I atm pressure

25°C and 2 atm pressure

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

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Remains constant

Increase

Decrease

Either increase or decrease

One Joule is equivalent to

Neutralization of acid-base is

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Spontaneous

Exothermic

Non spontaneous

Both "a" and "c

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

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

Most of the reactions which give stable products are

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Endothermic

Exothermic

Isothermal

Non of these

Which of the following has positive value of enthalpy

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Neutralisation

Atomization

combustion

All of the above

Which of the following enthalpy change always have a negative value

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∆Hf

∆H sol

∆Hc

∆Hat

In order to determine ∆H (latt) of ionic compound which is correct relationship

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∆H latt. = ∆Hf - ∆Hx

∆H latt. = ∆Ha + ∆Hv

∆H latt. = ∆Hf + ∆Hx

∆H latt. = ∆Hf - ∆H sol.

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