The magnitudes of enthalpy changes for irreversible adiabatic expansion of a gas from 1 L to 2 L is ΔH , and for reversible adiabatic expansion for the same expansion is ΔH 2 . Then

ΔH 1 = ΔH 2 , enthalpy being a state function ΔH 1 = ΔH 2

ΔH 1 = ΔE 1 and ΔH 2 = ΔE 2 where E 1 and E 2 are magnitudes of change in internal energy of gas in these expansions respectively.

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at 25 ° C is

298 × 10 7 × 8 . 31 × 2 . 303 log 2 .

2 . 303 × 298 × 0 . 082 log 2 .

2 . 303 × 298 × 0 . 082 log 0 . 5 .

8 . 31 × 10 7 × 298 × 2 . 303 log 0 . 5 .

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Which one of the following equations does not correctly represent the first law of thermodynamics for the given process in an ideal gas ?

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Important Questions on Thermodynamics

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 7

Consider the reaction at $300 K$

$H_{2} (g) + {Cl}_{2} (g) ⟶ 2 HCl (g); △ H ° = - 185 kJ$

If $2$ moles of $H_{2}$ completely react with $2$ mole of ${Cl}_{2}$ to form $HCl$ , what is $△ U °$ for this reaction.

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 8

A piece of ${NH}_{4} Cl$ is kept inside a balloon filled with some air, having thermally insulated walls. The temperature is kept just above sublimation temperature of ${NH}_{4} Cl$ .

${NH}_{4} Cl (s) \overset{sublime}{⟶} {NH}_{3} (g) + HCl (g)$ .

Which of the following is correct regarding this?

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 9

2

moles of an ideal gas is expanded isothermally and reversibly from

1

litre to

10

litre. Find the enthalpy change in

kJ {mol}^{- 1}

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 10

The magnitudes of enthalpy changes for irreversible adiabatic expansion of a gas from

1

L

2

L

ΔH

, and for reversible adiabatic expansion for the same expansion is

{ΔH}_{2}

. Then

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 11

A certain mass of gas is expanded from (

1

L

10

atm

) to (

4

L

5

atm

) against a constant external pressure of

1

atm

. If initial temperature of gas is

300

K

and the heat capacity of process

50

J / {}^{\circ}C

. Then the enthalpy change during the process is

(1 L atm ≃ 100 J)

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 12

A given mass of gas expands from the state $A$ to the state $B$ by three paths $1, 2$ and $3$ as shown in the figure. If $w_{1}, w_{2}$ and $w_{3}$ , respectively be the magnitudes work done by the gas alonq three paths then

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 13

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3.0 L, 95 K)

\to

(4.0 atm, 5.0 L, 245 K) with a change in internal energy,

Δ U

= 30.0 L atm. The change in enthalpy

(Δ H)

of the process in L atm is

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 2>Q 14

One mole of an ldeal monoatomic gas at temperature

T

and volume

1

L

expands to

2

L

against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:

Which one of the following equations does not correctly represent the first law of thermodynamics for the given process in an ideal gas ?

Important Questions on Thermodynamics

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