Question # 1

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

One kilo calorie is equal to

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4.184J

1000J

4184J

1kJ

Total heat content of a system is called

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Internal energy

Entropy

Enthalpy

All of these

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

The enthalpies of all elements in their standard states are

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Unity

always +ve

always -ve

zero

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.

A system absorbs 100 kJ heat and performs 50 kJ work on the surroundings. The increase in internal energy of the system is

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50kJ

100 kJ

150kJ

5000 kJ

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 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

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 enthalpy of formation of a compound is

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Positive

Either positive or negative

Negative

None

The enthalpy change for the reaction C2H2 + 5/2 O2 --------> 2CO2 + H2O is known as enthalpy of

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Fomation of CO2

Fusion ofC2H4

Combustion of C2H4

Vaporization of C2H2

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

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

Change in enthalpy (∆H) of a system can be calculated by

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∆H=∆E - PV

ΔH =ΔE +q

∆H = ∆E - q

∆Η = ΔΕ + P∆V

Which of the following enthalpy change always have a negative value

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∆Hf

∆H sol

∆Hc

∆Hat

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

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Zero

positive

Negative

Infinity

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

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

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