Question # 1

Which of the following enthalpy change always have a negative value

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∆Hf

∆H sol

∆Hc

∆Hat

The lattice energy of NaCl is

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787 j/ mole

790 kj/mol

780 kJ/ mol

-787 kI / mole

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

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

Born-Haber cycle is an application of

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Hess's law

1" law of thermodynamics

Avogadro's law

1law of thermochemistry

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 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

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

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

One Joule is equivalent to

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4.184 cal.

0.4184cal.

1/2 cal.

1/4.184 cal

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

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