Properties of...

Properties of Enthalpy

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Q. Heat of a reaction is defined as the amount of heat absorbed or evolved at a given temperature when the reactants have combined to form the products is represented by balanced chemical equation. If the heat is denoted by

q

then the numerical value of

q

depends on the manner in which
the reaction is performed for two methods of conducting chemical reactions in calorimeters.

The heat capacity of a bomb calorimeter is 300 J/K. When 0.16 gm of methane was burnt in this calorimeter, the temperature rose by

3^{\circ} C

. The value of

Δ U

per mole will be:

100 kJ
90 kJ
900 kJ
48 kJ

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Q. One mole of an ideal gas at

300 K

is expanded isothermally from an initial volume of

1

litre to

10

litres. The value of

△ U

for this process is:

(R = 2 {cal mol}^{- 1} K^{- 1})

$163.7 cal$
$0$
$138.1 cal$
$9 atm L$

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Q. Under which of the following conditions is the relation,

Δ H = Δ U + P Δ V

valid for a closed system.

At constant pressure
At constant volume
At constant temperature
At constant volume and pressure

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Q. The bond dissociation energies of

X_{2}

Y_{2}

and

X Y

are in the ratio of 1 : 0.5 : 1.

△ H

for the formation of

X Y

is –200 kJ

m o l^{- 1}

. The bond dissociation energy of

X_{2}

will be

800 kJ $m o l^{- 1}$
100 kJ $m o l^{- 1}$
200 kJ $m o l^{- 1}$
400 kJ $m o l^{- 1}$

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Q. The heat of atomization of a compound

X Y_{3}

in gaseous state is

E k J m o l^{- 1}

. What is the bond energy of

X - Y

bond in

k J m o l^{- 1}

unit?

$E$
$3 E$
$\frac{E}{3}$
$\frac{E}{6}$

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Q. When one mole of an ideal gas is compressed to half of the initial volume and simultaneously heated to twice of its initial temperature, the change in enthalpy