Question # 1

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.

The exothermic process is

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Evaporation

Sublimation

Respiration

Boiling

Which of the following has positive value of enthalpy

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Neutralisation

Atomization

combustion

All of the above

Enthalpy of a system can be calculated by which of following relationship

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q=ΔΕ

q=m×S×∆T

q=pv

q=m×v×∆T

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

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

Which of the following enthalpy change always have a negative value

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∆Hf

∆H sol

∆Hc

∆Hat

Neutralization of acid-base is

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Spontaneous

Exothermic

Non spontaneous

Both "a" and "c

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

How much heat is absorbed by 100 g of water when its temperature decreases from 25°C to 5°C? (heat capacity is 4.2 J/gK)

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84,000J

2000/4.2J

-2000/4.2j

-8400J

The lattice energy of NaCl is

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787 j/ mole

790 kj/mol

780 kJ/ mol

-787 kI / mole

The enthalpy change AH of a process is given by the relation

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ΔΗ =ΔΕ + P∆V

ΔH=ΔE +W

ΔH =ΔΕ-ΔnRT

ΔΕ =ΔΗ + P∆V

One kilo calorie is equal to

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4.184J

1000J

4184J

1kJ

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

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

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Zero

positive

Negative

Infinity

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

Decomposition of H2O is

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Endothermic reaction

Nuclear reaction

Exothermic reaction

Zero nuclear reaction

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

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

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

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

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