Question # 1

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

The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps.it is known as

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Henry's law

Hess's law

joule's law

Law of conservation of energy

Neutralization of acid-base is

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Spontaneous

Exothermic

Non spontaneous

Both "a" and "c

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

Most of the reactions which give stable products are

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Endothermic

Exothermic

Isothermal

Non 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

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

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

The lattice energy of NaCl is

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787 j/ mole

790 kj/mol

780 kJ/ mol

-787 kI / mole

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

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

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

One kilo calorie is equal to

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4.184J

1000J

4184J

1kJ

Decomposition of H2O is

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Endothermic reaction

Nuclear reaction

Exothermic reaction

Zero nuclear reaction

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

NaOH+HCI- NaCI+ H2O. Enthalpy change in the above reaction is called

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Enthalpy of reaction

Enthalpy of Neutralisation

Enthalpy of formation

Enthalpy of combustion

The change in enthalpy when one mole of a substance is dissolved in a specified quantity of solvent at a given temperature is called

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Heat of reaction

Heat of solvation

Heat of combustion

Heat of solvent

Enthalpy of a reaction can be measured by

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Glass calorimeter

Barometer

Manometer

Thermometer

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

Born-Haber cycle is an application of

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Hess's law

1" law of thermodynamics

Avogadro's law

1law of thermochemistry

The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called

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Heat of reaction

Heat of formation

Heat of atomization

Heat of combustion

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