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If $5$ moles of an ideal gas expands from $10 L$ to a volume of $100 L$ at $300 K$ under isothermal and reversible condition then work, $w$ , is $- x J$ . The value of $x$ is $-$ _______.

(Given $R = 8 .314 J K^{- 1} {mol}^{- 1}$ )

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Important Questions on Chemical Thermodynamics

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Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

A system consisting of 1 mol of an ideal gas undergoes a reversible process,

A \to B \to C \to A

(schematically indicated in the figure below). If the temperature at the starting point A is 300 K and the work done in the process

B \to C

is 1 L atm, the heat exchanged in the entire process in L atm is

Question Image

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

During the free expansion of an ideal gas in an isolated chamber,

MEDIUM

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

A thermodynamic cycle in the pressure

(P)

-volume

(V)

plane is given below:
Question Image

AB

and

CD

are isothermal processes while

BC

and

DA

are adiabatic processes. The same cycle in the temperature

(T)

- entropy

(S)

plane is :

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

An ideal gas undergoes isothermal compression from

5 m^{3}

1 m^{3}

against a constant external pressure of

4 N m^{- 2}

. The heat released in this process is

24 J {mol}^{- 1} K^{- 1}

and is used to increase the pressure of

1

mole of

Al

. The temperature of

Al

increases by:

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

Under the isothermal condition, a gas at $300 K$ expands from $0.1 L$ to $0.25 L$ against a constant external pressure of $2$ bar. The work done by the gas is

(Given that $1 L$ bar $= 100 J$ )

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

Three mole of an ideal gas expand isothermally and reversibly from

10 m^{3}

20 m^{3}

300 K,

calculate the work done?

(R = 8.314 J K^{- 1} {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

An ideal gas initially at temperature, pressure and volume,

27 ° C, 1.00

bar and

10 L

respectively is heated at constant volume until pressure is

10.0

bar, it then undergoes a reversible isothermal expansion until pressure is

1.00 bar,

what is the total work

W

, during this process?

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

Consider the reversible isothermal expansion of an ideal gas in a closed system at two different temperatures

T_{1}

and

T_{2} (T_{1} < T_{2})

. The correct graphical depiction of the dependence of work done

(w)

vs the final volume

(V)

is:

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

The work done in

ergs

for the reversible expansion of one

mole

of an ideal gas from a volume of

10 litres

20 litres

25 ° C

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

How much heat will be absorbed by $1$ mole of an ideal gas, if it is expanded reversibly from $5 L$ to $25 L$ at $27^{o} C$ ?

$(\log 3 = 0.5, \log 4 = 0.6, \log 5 = 0.7)$

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

Which of the following relation is not correct?

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

The volume vs. temperature graph of 1 mole of an ideal gas is given below

Question Image

The pressure of the gas (in atm) at

X, Y

and

Z,

respectively, are

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

For $1 mol$ of gas, the plot of $pV$ vs $p$ is shown below. p is the pressure and $V$ is the volume of the gas.

Question Image

What is the value of compressibility factor at point $A$ ?

MEDIUM

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

The combination of plots which does not represent isothermal expansion of an ideal gas is

$(A)$ Question Image

$(B)$

$(C)$

$(D)$

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

An ideal gas undergoes a cyclic process as shown in the figure
Question Image

∆ U_{BC} = - 5 {KJmol}^{- 1}, q_{AB} = 2 {KJmol}^{- 1}

W_{AB} = - 5 {KJmol}^{- 1}, W_{CA} = 3 {KJmol}^{- 1}

Heat absorbed by the system during process

CA

HARD

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

A cylinder containing an ideal gas (

0.1 m o l

1.0 d m^{3}

) is in thermal equilibrium with a large volume of

0.5

molal aqueous solution of ethylene glycol at its freezing point. If the stoppers

S_{1}

and

S_{2}

(as shown in the figure) are suddenly withdrawn, the volume of the gas in litres after equilibrium is achieved will be _____________.
(Given,

K_{f} (w a t e r) = 2.0 K k g m o l^{- 1}, R = 0.08 d m^{3} a t m K^{- 1} m o l^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

The magnitude of work done by a gas that undergoes a reversible expansion along the path $A B C$ shown in the figure is _________.
Question Image

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

An ideal gas expands adiabatically against vacuum. Which of the following is correct for the given process?

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

100 mole

H_{2} O_{2}

decompose at

1 bar

and

300 K

, the work is done (

kJ

) by one mole of

O_{2} (g)

as it expands against

1 bar

pressure is:

2 H_{2} O_{2} (l) ⇌ 2 H_{2} O (l) + O_{2} (g)

(R = 8 .3 J K^{- 1} {mol}^{- 1})

EASY

Chemistry>Physical Chemistry>Chemical Thermodynamics>Applications of First Law of Thermodynamics

An ideal gas undergoes isothermal expansion at constant pressure. During the process:

If 5 moles of an ideal gas expands from 10L to a volume of 100L at 300K under isothermal and reversible condition then work, w, is −x J. The value of x is -_______. (Given R=8.314 J K-1 mol-1)

Important Questions on Chemical Thermodynamics

Learn and Prepare for any exam you want !

If $5$ moles of an ideal gas expands from $10 L$ to a volume of $100 L$ at $300 K$ under isothermal and reversible condition then work, $w$ , is $- x J$ . The value of $x$ is $-$ _______.

(Given $R = 8 .314 J K^{- 1} {mol}^{- 1}$ )