NCERT Solutions For Class 11 Physics Chapter 11 Thermodynamics - 2025-26

1. A geyser heats water flowing at the rate of \[3.0\] litres per minute from \[27{}^\circ C\] to \[77{}^\circ C\]. If the geyser operates on a gas burner, what is the rate of consumption of the fuel if its heat of combustion is \[4.0\times {{10}^{4}}J/g\]  ?

Ans: It is provided that,

Water flows at a rate of \[3.0\] litre/min \[=3\times {{10}^{-3}}{{m}^{3}}/\min \]

Density of water, \[\rho ={{10}^{3}}kg/{{m}^{3}}\].

Clearly, mass of water flowing per minute \[=3\times {{10}^{-3}}\times {{10}^{3}}kg/\min =3kg/\min \]

The geyser heats the water, raising the temperature from \[27{}^\circ C\] to \[77{}^\circ C\].

Initial temperature, \[{{T}_{1}}=27{}^\circ C\]

Final temperature, \[{{T}_{2}}=77{}^\circ C\]

Thus, rise in temperature,

\[\Delta T={{T}_{2}}-{{T}_{1}}\]

\[\Rightarrow \Delta T=77{}^\circ C-27{}^\circ C\]

\[\Rightarrow \Delta T=50{}^\circ C\]

Now, heat of combustion \[=4\times {{10}^{4}}J/g=4\times {{10}^{7}}J/kg\]

Specific heat of water \[=4.2J/g\,{}^\circ C\]

It is known that total heat used, \[\Delta Q=mc\Delta T\]

\[\Rightarrow \Delta Q=3\times 4.2\times {{10}^{3}}\times 50\]

\[\Rightarrow \Delta Q=6.3\times {{10}^{5}}J/\min \]

Now, consider \[m\]kg of fuel to be used per minute.

Thus, the heat produced \[=m\times 4\times {{10}^{7}}J/\min \]

However, the heat energy taken by water \[=\] heat produced by fuel

Thus, equating both the sides,

\[\Rightarrow 6.3\times {{10}^{5}}=m\times 4\times {{10}^{7}}\]

\[\Rightarrow m=\frac{6.3\times {{10}^{5}}}{4\times {{10}^{4}}}\]

\[\Rightarrow m=15.75\,g/\min \]

Clearly, the rate of consumption of the fuel when its heat of combustion is \[4.0\times {{10}^{4}}J/g\] supposing the geyser operates on a gas burner is \[15.75\,\,g/\min \].

2. What amount of heat must be supplied to \[2.0\times {{10}^{-2}}kg\] of Nitrogen (at room temperature) to raise its temperature by \[45{}^\circ C\] at constant pressure? (Molecular mass of \[{{N}_{2}}=28\]; \[R=8.3J\,mo{{l}^{-1}}{{K}^{-1}}\].)

Ans: Provided that,

Mass of Nitrogen, \[m=2.0\times {{10}^{-2}}kg=20g\].

Rise in temperature, \[\Delta T=45{}^\circ C\].

Molecular mass of \[{{N}_{2}}\], \[M=28\]

Universal gas constant, \[R=8.3J\,mo{{l}^{-1}}{{K}^{-1}}\].

Number of moles, \[n=\frac{m}{M}\]

\[\Rightarrow n=\frac{2\times {{10}^{-2}}\times {{10}^{3}}}{28}\]

\[\Rightarrow n=0.714\]

Now, molar specific heat at constant pressure for nitrogen,

\[{{C}_{p}}=\frac{7}{2}R\]

\[\Rightarrow {{C}_{p}}=\frac{7}{2}\times 8.3\]

\[\Rightarrow {{C}_{p}}=29.05J\,mo{{l}^{-1}}{{K}^{-1}}\]

The total amount of heat to be supplied is given by the relation:

\[\Delta Q=n{{C}_{p}}\Delta T\]

\[\Rightarrow \Delta Q=0.714\times 29.05\times 45\]

\[\Rightarrow \Delta Q=933.38J\]

Clearly, the amount of heat to be supplied is \[933.38J\].

3. Explain why

(a) Two bodies at different temperatures \[{{T}_{1}}\]and \[{{T}_{2}}\] if brought in thermal contact do not necessarily settle to the mean temperature.

Ans: If two bodies at different temperatures \[{{T}_{1}}\]and \[{{T}_{2}}\] are brought in thermal contact, heat is said to flow from the body at higher temperature to the body at lower temperature until an equilibrium is obtained, i.e., until a point at which the temperatures of both the bodies becomes the same. 

The equilibrium temperature turns out to be the same as the mean temperature, which can be denoted as  \[\frac{\left( {{T}_{1}}+{{T}_{2}} \right)}{2}\] only when thermal capacities of the two bodies are the same.

(b) The coolant in a chemical or a nuclear plant (i.e., the liquid used to prevent the different parts of a plant from getting too hot) should have high specific heat.

Ans: The coolant in a chemical or nuclear plant must have a high specific heat as it is known that higher the specific heat of the coolant, higher is its heat-absorbing capacity and vice-versa.

Thus, a liquid which has a high specific heat is the best coolant to be utilized in a nuclear or chemical plant. This prevents different parts of the plant from becoming too hot.

(c) Air pressure in a car tyre increases during driving.

Ans: When the car is in motion, the temperature of air inside the tyre rises due to motion of the air molecules. Charle’s law suggests that pressure is directly proportional to the temperature, \[P\propto T\].

Clearly, when the temperature inside a tyre rises, the air pressure inside the tyre would also increase.

(d) The climate of a harbour town is more temperate than that of a town in a desert at the same latitude.

Ans:  A harbour town has a more temperate climate than a town located in a desert at the same latitude. 

In a harbour town, the relative humidity is greater than that in a desert town.

4. A cylinder with a movable piston contains \[3\] moles of hydrogen at standard temperature and pressure. The walls of the cylinder are made of a heat insulator, and the piston is insulated by having a pile of sand on it. By what factor does the pressure of the gas increase if the gas is compressed to half its original volume?

Ans: Here, the cylinder is said to be completely insulated from its neighbourhood. As a result, no heat gets exchanged between the system (cylinder) and its neighbourhood. Clearly, the process turns out to be adiabatic.

Now, consider:

Initial pressure inside the cylinder \[={{P}_{1}}\]

Final pressure inside the cylinder \[={{P}_{2}}\]

Initial volume inside the cylinder \[={{V}_{1}}\]

Final volume inside the cylinder \[={{V}_{2}}\]

Ratio of specific heats, \[\gamma =1.4\]

For an adiabatic process, it is known that \[{{P}_{1}}{{V}^{\gamma }}_{1}={{P}_{2}}{{V}_{2}}^{\gamma }\].

Also, the final volume is compressed to half of its initial volume.

\[\Rightarrow {{V}_{2}}=\frac{{{V}_{1}}}{2}\]

Thus,

\[\Rightarrow {{P}_{1}}{{V}^{\gamma }}_{1}={{P}_{2}}{{\left( \frac{{{V}_{2}}}{2} \right)}^{\gamma }}\].

\[\Rightarrow \frac{{{P}_{2}}}{{{P}_{1}}}=\frac{{{V}_{1}}^{\gamma }}{{{\left( \frac{{{V}_{1}}}{2} \right)}^{\gamma }}}\]

\[\Rightarrow \frac{{{P}_{2}}}{{{P}_{1}}}={{2}^{\gamma }}={{2}^{1.4}}=2.639\]

Clearly, the pressure rises by a factor of \[2.639\].

5. In changing the state of a gas adiabatically from an equilibrium state A to another equilibrium state B, an amount of work equal to \[22.3J\] is done on the system. If the gas is taken from state A to B via a process in which the net heat absorbed by the system is \[9.35\,cal\], how much is the net work done by the system in the latter case? (Take \[1\,cal=4.19J\] )

Ans: It is provided that the work done \[\left( W \right)\] on the system when the gas transforms from state A to state B is \[22.3J\].

This is an adiabatic process. Thus, the change in heat is zero.

\[\Rightarrow \Delta Q=0\]

(As the work is done on the system)

Using the first law of thermodynamics,

\[\Delta Q=\Delta U+\Delta W\]

where,

\[\Delta U=\] change in the internal energy of the gas

When the gas transforms from state A to state B via a process, the net heat absorbed by the system is given by

\[\Delta Q=9.35cal=9.35\times 4.19J=39.1765J\]

Heat absorbed can be given by the equation,

\[\Delta Q=\Delta U+\Delta W\]

\[\Rightarrow \Delta W=\Delta Q-\Delta U=39.1765-22.3=16.8765J\]

Clearly, \[16.88J\] of work is done by the system.

6. Two cylinders $A$ and $B$ of equal capacity are connected to each other via a stopcock. \[A\]contains a gas at standard temperature and pressure. \[B\] is completely evacuated. The entire system is thermally insulated. The stopcock is suddenly opened. Answer the following:

(a) What is the final pressure of the gas in \[A\]and \[B\]?

Ans: The volume which can be availed by the gas at $1$ atmospheric pressure would be doubled when the stopcock is opened instantly. 

As volume is inversely proportional to pressure, the pressure reduces to one-half times its original value. 

The initial pressure of the gas being \[1\]atm results in the pressure of each cylinder to be \[0.5\]atm.

(b) What is the change in internal energy of the gas?

Ans: Change in the internal energy of any gas occurs when work is done by or on the gas. 

Here, as no work is done by or on the gas and thus, the internal energy of the gas would not change. Clearly, the change in internal energy of the gas is \[0\].

(c) What is the change in the temperature of the gas?

Ans: Change in the temperature of any gas occurs when work is done by or on the gas. 

Here, as no work is done by the gas during the expansion of the gas, the temperature of the gas would not change. Clearly, the change in temperature of the gas is \[0\].

(d) Do the intermediate states of the system (before settling to the final equilibrium state) lie on its P-V-T surface?

Ans: No, the intermediate states of the system do not lie on the P-V-T surface since the process of free expansion is rapid and cannot be limited.

The intermediate states are non-equilibrium states and do not follow the gas equation. In due course of time, the gas returns to its original state.

7. A steam engine delivers \[5.4\times {{10}^{8}}J\] of work per minute and services \[3.6\times {{10}^{9}}J\] of heat per minute from its boiler. What is the efficiency of the engine? How much heat is wasted per minute?

Ans: Provided that,

Work done by the steam engine per minute, \[W=5.4\times {{10}^{8}}J\]

Heat supplied from the boiler, \[H=3.6\times {{10}^{9}}J\]

\[Efficiency\,of\,the\,engine=\frac{Output\,Energy}{Input\,Energy}\]

\[\Rightarrow \eta =\frac{W}{H}\]

\[\Rightarrow \eta =\frac{5.4\times {{10}^{8}}}{3.6\times {{10}^{9}}}\]

\[\Rightarrow \eta =0.15\]

Thus, the percentage efficiency of the engine is \[15%\].

Amount of heat wasted \[=3.6\times {{10}^{9}}-5.4\times {{10}^{8}}=30.6\times {{10}^{8}}=3.06\times {{10}^{9}}J\]

Clearly, the amount of heat wasted per minute is \[3.06\times {{10}^{9}}J\].

8. An electric heater supplies heat to a system at a rate of \[100W\]. If the system performs work at a rate of \[75\] Joules per second. At what rate is the internal energy increasing?

Ans: It is provided that,

Heat is supplied to the system by an electric heater at a rate of \[100W\]. 

Thus, heat supplied, \[Q=100J/s\]

The system operates at a rate of \[75J/s\]. 

Clearly, work done, \[W=75J/s\]

Using the first law of thermodynamics,

\[Q=U+W\]

where, 

\[U=\]internal energy 

\[\Rightarrow U=Q-W\]

\[\Rightarrow U=100-75\]

\[\Rightarrow U=25J/s\]

\[\Rightarrow U=25W\] 

Clearly, the internal energy of the given electric heater rises at a rate of \[25W\]or \[25J/s\].

9. A thermodynamic system is taken from an original state to an intermediate state by the linear process shown in figure

Its volume is then reduced to the original value from\[E\] to \[F\] by an isobaric process. Calculate the total work done by the gas from \[D\] to \[E\] to \[F\].

Ans: Considering the given linear process in a thermodynamic system, it can be understood that,

Total work done by the gas from \[D\] to \[E\] to \[F\] is equal to the area of \[\Delta DEF\].

Area of \[\Delta DEF\] \[=\frac{1}{2}\times DE\times EF\]

where, 

\[DF=\] Change in pressure 

\[\Rightarrow DF=600N/{{m}^{2}}-300N/{{m}^{2}}\]

\[\Rightarrow DF=300N/{{m}^{2}}\]

Also,

\[FE=\]Change in volume $=5-2=3{{m}^{3}}$

Thus,

Area of \[\Delta DEF\]\[=\frac{1}{2}\times 300\times 3=450J\]  

Clearly, the total work done by the gas from \[D\]to \[E\] to \[F\]is \[450J\].

10. A refrigerator is to maintain eatables kept inside at \[9{}^\circ C\]. If room temperature is \[36{}^\circ C\], calculate the coefficient of performance. 

Ans: Here, the temperature inside the refrigerator can be provided as,

\[{{T}_{1}}=9{}^\circ C=282K\]

Room temperature is given as,

\[{{T}_{2}}=36{}^\circ C=309K\]

Coefficient of performance can be given by the relation,

\[COP=\frac{{{T}_{1}}}{\left( {{T}_{2}}-{{T}_{1}} \right)}\]

\[\Rightarrow COP=\frac{282}{\left( 309-282 \right)}\]

\[\Rightarrow COP=10.44\] 

Clearly, the coefficient of performance of the mentioned refrigerator is \[10.44\].

Thermodynamics Physics Class 11 Ncert Solutions PDF

Physics, the study of matter, motion, energy and behaviour of space and time requires thorough reading and understanding. The topic of Thermodynamics Class 11 Physics contains critical sub-topics like thermal equilibrium, state variables, quasistatic process, sign convention, adiabatic, etc.

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NCERT Solutions Class 11 Physics Thermodynamics

Thermodynamics Class 11 Physics solution contains ten questions both in theory and equations. Check the explanations below.

1. Thermodynamics Physics Class 11

Solution - In this question, students need to determine the rate of fuel consumption if the heat of combustion is 4.0 × 10⁴ J/g. Here the geyser heats 3.0ltr water from 27 °C to 77 °C.

2. Class 11 Physics Thermodynamics

Solution - This question requires a student to find the amount of heat supplied to 2.0 × 10 square kg of nitrogen. Its temperature is raised by 45 °C at constant pressure.

3. Thermodynamics Class 11 Physics NCERT Solutions

Solution - The third question from Thermodynamics Class 11 Physics contains a question asking students to explain how two bodies at a temperature, when brought in thermal contact, do not settle to mean temperature. Other questions are why a coolant in a nuclear reactor must have specific heat. Air pressure in car tyres increases during driving and the climate of harbour town is more than desert is also needed to be explained.

4. NCERT Solutions Class 11 Physics Thermodynamics

Solution - This fourth question requires a student to calculate the pressure of a gas when the cylinder gas with a movable piston containing 3 moles of hydrogen is compressed to half. Here the walls of the cylinder are insulated with sand.

5. Ch 11 Physics Class 11

Solution - A student needs to calculate how much work is done by a system where the gas changes from equilibrium state A to B is 22.3 J. Here ∆Q is zero, and the net heat absorbed by the system is 9.35 cal.

6. Thermodynamics Class 11 NCERT Solutions Physics

Solution - In this question from Thermodynamics class 11 Physics, two cylinders A and B are connected by a stopcock where A is filled with gas while B is empty. The entire system is insulated when the stopcock is opened. A student needs to find absolute pressure of A and B, change of internal pressure, the temperature of a gas and intermediate state of systems.

7. Thermodynamics Physics Class 11 NCERT Solutions PDF

Solution - In this seventh question, a steam engine delivers 5.4 × 10⁸ J of work per minute and services 3.6 × 10⁹ J. Here a student needs to calculate efficiency of engine and heat wasted per minute.

8. Class 11 Physics Chapter 11 NCERT Solutions

Solution - Here, the rate of internal energy increases when an electric heater supplies heat to a system that is 100 w and how the system works at a rate of 75 Joules per second.

9. CBSE Class 11 Physics Thermodynamics NCERT Solutions

Solution - In the ninth question, a figure is given where the thermodynamics is in an original state to an intermediate state by the linear process. When volume is reduced from E to F, the total work done is needed to be calculated by students.

10. Class 11th Physics Thermodynamics NCERT Solution

Solution - This tenth question asks a student to calculate the coefficient of performance when a refrigerator with eatables has a temperature of 9°C, and room temperature is 36°C.

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