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

Enthalpy of a reaction can be measured by

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Glass calorimeter

Barometer

Manometer

Thermometer

Neutralization of acid-base is

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Spontaneous

Exothermic

Non spontaneous

Both "a" and "c

The enthalpy of formation of a compound is

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Positive

Either positive or negative

Negative

None

Choose from the followings the correct statement about Born Haber cycle

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Born Haber cycle is different from Hess's law

The energy changes in a cyclic process is not zero

The lattice energy of crystalline substances can be calculated easily

None

Enthalpy of neutralization (∆H°n) per mole of H2SO4/ Ba(OH)2 is

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+57.4 kJmol-1

-114.8 kJmol-1

-57.4 kJmol-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

Most of the reactions which give stable products are

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Endothermic

Exothermic

Isothermal

Non of these

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

Decomposition of H2O is

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Endothermic reaction

Nuclear reaction

Exothermic reaction

Zero nuclear reaction

Hess's law is analogous to

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Law of heat summation

law of increasing entropy

Law of heat exchange

Ist law of thermodynamics

Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called

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Gibb's energy

Bond energy

Lattice energy

A state function which describes together the internal energy and product of pressure and volume is called

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Enthalpy

internal energy

Work

Kinetic energy

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

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

Total heat content of a system is called

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Internal energy

Entropy

Enthalpy

All of these

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 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

The exothermic process is

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Evaporation

Sublimation

Respiration

Boiling

For an endothermic reaction, enthalpy of reactants

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Is smaller than that of the products

Is greater than that of the products

Must be greater or smaller than that of the products

Is equal to that of the products

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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