A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 3 7 . 0 ∘ C . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be (R = 8.314 J/mol K) (ln7.5 = 2.01)

q = + 2 0 8 J , w ⁡ = - 2 0 8 J

q = + 2 0 8 J , w ⁡ = + 2 0 8 J

q = - 2 0 8 J , w ⁡ = - 2 0 8 J

HARD

Earn 100

$1 mole$ of an ideal gas, $[γ = 1.5]$ , are taken through a series of processes.

Information-I The temperature at state ' $A$ ' is $300 K$ .

Information-II The reversible isothermal expansion from $B to C$ doubles the volume.

Information-III The entropy change of the system from $C to D$ is $4 \ln 16 cal K^{- 1}$ .

Select the correct option(s) using the above information.

11.11% studentsanswered this correctly

Important Questions on Thermodynamics

MEDIUM

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

A reversible cyclic process for an ideal gas is shown below. Here,

P, V, a n d T

are pressure, volume and temperature, respectively. The thermodynamic parameters

q, w, H a n d U

are heat, work, enthalpy and internal energy, respectively.

Question Image

The correct option(s) is (are)

HARD

Chemistry>Physical Chemistry>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>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:

MEDIUM

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

The magnitude of reversible work done by an ideal gas in four different processes: isothermal expansion, adiabatic expansion, constant pressure expansion, and free expansion are

W_{i}, W_{a}, W_{p}

, and

W_{f}

respectively. Choose the right order of sequence for the magnitude of the work done. (Change in the volume is same for all the processes.)

MEDIUM

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

The qualitative sketches I, II and III given below show the variation of surface tension with molar concentration of three different aqueous solutions of KCl,

C H_{3} O H

and

C H_{3} {(C H_{2})}_{11} O S O_{3}^{-} N a^{+}

at room temperature. The correct assignment of the sketches is -

Question Image

HARD

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

One mole of an ideal monoatomic gas is subjected to changes as shown in the graph. The magnitude of the work done (by the system or on the system) is _______ J (nearest integer)

Question Image

Given : log 2 = 0.3, ln 10 = 2.3

EASY

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

Calculate the work done during compression of

2

mol of an ideal gas from a volume of

1 m^{3}

10

{dm}^{3}

300 K

against a pressure of

100 kPa

HARD

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

Which of the following

p - V

curve represents maximum work done?

MEDIUM

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

$State 1 ⇆ State 2 ⇆ State 3 (\begin{matrix} T = 300 K \\ P = 15 bar \\ 1 mole \end{matrix}) (\begin{matrix} T = 300 K \\ P = 10 bar \\ 1 mole \end{matrix}) (\begin{matrix} T = 300 K \\ P = 5 bar \\ 1 mole \end{matrix})$

Above shows a cyclic process. Calculate the total work done during one complete cycle.
(Assume a single step to reach the next state).

HARD

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

The above

P - V

diagram represents the thermodynamic cycle of an engine, operating with an ideal mono-atomic gas. The amount of heat, extracted from the source in a single cycle, is:

MEDIUM

Chemistry>Physical Chemistry>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

MEDIUM

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

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of

37 . 0^{\circ} C

. As it does so, it absorbs 208 J of heat. The values of q and w for the process will be
(R = 8.314 J/mol K) (ln7.5 = 2.01)

EASY

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

A piece of ice falls from a height

h

so that it melts completely. Only one-quarter of the heat produced is absorbed by the ice and all energy of ice gets converted into heat during its fall. The value of

h

is:
(Latent heat of ice is

3.4 \times 10^{5} {J kg}^{- 1}

and

g = 10 {N kg}^{- 1}

)

EASY

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

The work done during combustion of

9 \times 10^{- 2}

kg

of ethane,

C_{2} H_{6} (g)

300 K

is (Given

R = 8 .314 {JK}^{- 1} {mol}^{- 1}

, atomic mass

C = 12, H = 1

)

EASY

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

A gas undergoes change from state

A

to state

B

. In this process, the heat absorbed and work done by the gas is

5 J and 8 J

, respectively. Now gas is brought back to

A

by another process during which

3 J

of heat is evolved. In this reverse process of

B to A

MEDIUM

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

X g

of ice at

0^{o} C

is added to 340g of water at

20^{o} C

. The final temperature of the resultant mixture is

5^{o} C

. The value of

X

(in g) is closest to

[Heat of fusion of ice

= 333 J / g

; Specific heat of water

= 4.184 J / g . K

]

MEDIUM

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

A certain mass of a gas was brought from state $A$ to $B$ by following three different paths, namely $1, 2$ and $3$ , respectively. Which of the following relations is correct for the work done?

Question Image

MEDIUM

Chemistry>Physical Chemistry>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>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

Important Questions on Thermodynamics

Learn and Prepare for any exam you want !