NCERT Solutions for Class 11 Physics Chapter 11 Thermodynamics

Q11.1 A geyser heats water flowing at the rate of 3.0 litres per minute from 27 °C to 77 °C. If the geyser operates on a gas burner, what is the rate of consumption of the fuel if its heat of combustion is $4.0\times {10}^4\mathrm{J}/\mathrm{g}$?

Answer:

The volumetric flow of water is

$\frac{dV}{dt}=3litresminut{e}^{-1}$

Density of water = 1000 g/litre

The mass flow rate of water is

$\frac{dm}{dt}=\rho \frac{dV}{dt}$
$\frac{dm}{dt}=3000gmi{n}^{-1}$

Specific heat of water, c = 4.2 J g -1 o C -1

The rise in temperature is $\mathrm{\Delta }T=77-27=50{}^{o}C$

The rate of energy consumption will be

$\frac{dQ}{dt}=\frac{dm}{dt}c\mathrm{\Delta }T$
$\frac{dQ}{dt}=3000\times 4.2\times 50$
$\frac{dQ}{dt}=6.3\times {10}^{5}Jmi{n}^{-1}$

The heat of combustion of fuel $=4.0\times {10}^{4}J/g$

The rate of consumption of fuel is

$$\begin{gathered} \frac{6.3\times {10}^5}{4\times {10}^4} \\ =15.75gmi{n}^{-1} \end{gathered}$$

Q11.2 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 °C at constant pressure? (Molecular mass of $N=28;R=8.3Jmo{l}^{-1}{K}^{-1}$ .)

Answer:

Mass of nitrogen, $m=2.0\times {10}^{-2}kg=20g$

Molar Mass of nitrogen, M N = 28 g

The number of moles is n

$n=\frac{m}{M_N}$
$n=\frac{20}{28}$
$n=0.714$

As nitrogen is a diatomic gas, it's molar specific heat at constant pressure C P is as follows

${C}_P=\frac{7R}{2}$
$C_P=\frac{7\times 8.3}{2}$
$C_P=29.05Jmo{l}^{-1}{}^o{C}^{-1}$

Rise in temperature, $\mathrm{\Delta }T={45}^o{C}^{-1}$

The amount of heat Q that must be supplied is

$Q=n{C}_P\mathrm{\Delta }T$
$Q=0.714\times 29.05\times 45$
$Q=933.38J$

Q11.3 (a) 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 $(T_1+T_2)/2$ .

Answer:

As we know, heat will flow from the hotter body to the colder body till their temperatures become equal. That temperature will be equal to the mean of the initial temperatures of the bodies only if the two thermal capacities of the two bodies are equal.

Q11.3 (b) Explain why

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.

Answer:

The coolant should have high specific heat so that it can absorb large amounts of heat without itself getting too hot and its temperature lies in the permissible region. The higher the specific heat, the more heat will be absorbed by the same amount of the material for a given increase in temperature.

Q11.3(c) Explain why

Air pressure in a car tyre increases during driving.

Answer:

As the car is driven, the air inside the tyre heats due to frictional forces. Thus, the temperature of the air inside the tyre increases and this, in turn, increases the pressure inside the tyre.

Q11.3 (d) Explain why

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

Answer:

The climate of a harbour town is more temperate than that of a town in a desert at the same latitude because of the formation of sea breezes.

Q11.4 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?

Answer:

As the walls of the cylinder and the piston are insulated, the process will be adiabatic. i.e. $P{V}^{\gamma }$ would be constant.

Hydrogen is a diatomic gas and therefore $\gamma =1.4$

Let the initial and final pressure be P 1 and P 2, respectively.

Let the initial and final volume be T 1 and T 2, respectively.

${P}_1{V}_1^{\gamma }=P_2{V}_2^{\gamma }$
$\frac{P_2}{P_1}={\left(\frac{V_1}{V_2}\right)}^{\gamma }$
$\frac{P_2}{P_1}=2^{1.4}$
$\frac{P_2}{P_1}=2.639$

The pressure thus increases by a factor 2.639

Q11.5 In changing the state of a gas adiabatically from an equilibrium state A to another equilibrium state B, an amount of work equal to 22.3 J 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 $1cal=4.19J$ )

Answer:

In the first case, the process is adiabatic, i.e. $\mathrm{\Delta }Q=0$

22.3 J work is done on the system, i.e. $\mathrm{\Delta }w=-22.3J$

$\mathrm{\Delta }Q=\mathrm{\Delta }u+\mathrm{\Delta }w$

$0=\mathrm{\Delta }u-22.3$

$\mathrm{\Delta }u=22.3J$

Since in the latter process as well,l the initial and final states are the same as those in the former process, $\mathrm{\Delta }u$ will remain the same for the latter case.

In the latter case, the net heat absorbed by the system is 9.35 cal

$\mathrm{\Delta }Q=9.35\times 4.2$
$\mathrm{\Delta }Q=39.3J$

$\mathrm{\Delta }w=\mathrm{\Delta }Q-\mathrm{\Delta }u$

$\mathrm{\Delta }w=39.3-22.3$

$\mathrm{\Delta }w=17.0J$

The network done by the system in the latter case is 17.0 J

Q11.6 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 ?

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

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

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

Answer:

As the entire system is thermally insulated and as free expansion will be taking place the temperature of the gas remains the same. Therefore PV is constant.

Initial Pressure P 1 = 1 atm

Initial Volume, V 1 = V

Final Volume, V 2 = 2V

Final Pressure P 2 will be

$$\begin{gathered} {P}_2=\frac{P_1{V}_1}{V_2} \\ {P}_2=\frac{P_1}{2} \\ {P}_2=0.5atm \end{gathered}$$

The final pressure of the gas in A and B is 0.5 atm.

b) Since the temperature of the gas does not change, its internal energy would also remain the same.

c) As the entire system is thermally insulated and as free expansion will be taking place the temperature of the gas remains the same.

d) The intermediate states of the system do not lie on its P-V-T surface as the process is a free expansion, it is rapid and the intermediate states are non-equilibrium states.

Q11.7 An electric heater supplies heat to a system at a rate of 100W. If system performs work at a rate of 75 joules per second. At what rate is the internal energy increasing?

Answer:

The rate at which heat is supplied $\mathrm{\Delta }Q=100W$

The rate at which work is done $\mathrm{\Delta }W=75J{s}^{-1}$

The rate of change of internal energy is $\mathrm{\Delta }u$

$$\begin{gathered} \mathrm{\Delta }u=\mathrm{\Delta }Q-\mathrm{\Delta }w \\ \mathrm{\Delta }u=100-75 \\ \mathrm{\Delta }u=25J{s}^{-1} \end{gathered}$$

The internal energy of the system is increasing at a rate of 25 J s -1

Q11.8 A thermodynamic system is taken from an original state to an intermediate state by the linear process shown in Fig. (12.13)

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

Answer:

The work done by the gas as it goes from state D to E to F is equal to the area of triangle DEF

DF is change in pressure = 300 N m -2

FE is change in Volume = 3 m 3

$area(DEF)=\frac{1}{2}\times DF\times FE$

$area(DEF)=\frac{1}{2}\times 300\times 3$

$area(DEF)=450J$

The work done is, therefore, 450 J.

Class 11 Physics NCERT Chapter 11: Higher Order Thinking Skills (HOTS) Questions

Q.1 Three moles of an ideal gas being initially at a temperature $T_0=273K$ were isothermally expanded to n = 5.0 times its initial volume and then isochorically heated so that the pressure in the final state becomes equal to that in the initial state. The total amount of heat transferred to the gas during the process equals Q = 80 kJ. Find the ratio $\gamma =C_p/C_v$ for this gas.

Answer:

$Q=Q_1+Q_2$

where
$Q_1\Rightarrow$ for Isothermal process
$Q_2\Rightarrow$ for Isochoric process

$Q=n^{\prime }\mathrm{R}{T}_0\log \frac{n{V}_0}{V_0}+n^{\prime }{C}_V(T_C-T_B)$

As $T_C=n{T}_0$ (If volume is made n times)

$Q=n^{\prime }\mathrm{R}{T}_0\log n+\gamma (n-1)T_0$

$\therefore \gamma =[1+\frac{n-1}{\frac{Q}{n^{\prime }R{T}_0}-\log n}]$

Putting the values

(Given n' = 3, n = 5)

$\gamma =1.4$

Hence, the answer is 1.4.

Q.2 In a pressure cooker, a sample of hydrogen gas was at a pressure of 1 atm. The volume of the cooker is 500 mL and mass of the cooker whistle is 100 g and it has a cross-section area of $0.1c{m}^2$. Its initial temperature is 27°C. Select the correct option(s):

a) The final temperature of the gas if the gas can lift the whistle, is 327°C
b) The final temperature of the gas if the gas can lift the whistle, is 227°C
c) The pressure required to lift the whistle is $2\times {10}^5$Pa
d) The pressure required to lift the whistle is ${10}^5$Pa

Answer:

The initial temperature of hydrogen, $T_1=273+27=300\mathrm{K}$
Initial pressure of hydrogen, $P_1=1\mathrm{atm}={10}^5\mathrm{Pa}$

$\begin{array}{rl}& P_2=P_0+\frac{mg}{A}\\ & ={10}^5+\frac{100\times {10}^{-3}}{0.01\times {10}^{-4}}\\ & =2\times {10}^5\end{array}$

As the volume is constant, we can use Gay Lussac's law:

$\frac{P_1}{T_1}=\frac{P_2}{T_2}\Rightarrow T_2=T_1\times \frac{P_2}{P_1}=300\times \frac{2}{1}=600\mathrm{K}=600-273={327}^{\circ }\mathrm{C}$

Hence, the answer is the option (a),(c).
Q.3 The volume of a gas is compressed adiabatically from state $V_1=7{\mathrm{m}}^3$ at a pressure of $2..4\times {10}^5\mathrm{N}{\mathrm{m}}^{-2}$ to the volume $V_2=0.875{\mathrm{m}}^3$. If the same compression is performed isothermally, calculate the difference in work done (in ${10}^5$ joule) in both processes. It is given that $\mathrm{y}=$ 1.67.

Answer:

$V_1=7{\mathrm{m}}^3,P_1=2.4\times {10}^5{\mathrm{Nm}}^{-2},V_2=0.875{\mathrm{m}}^3$

In adiabatic process

$\begin{array}{rl}& P_1{V}_1^{\gamma }=P_2{V}_2^{\gamma }\\ & \Rightarrow P_2=2.4\times {10}^5{\left[\frac{7}{0.875}\right]}^{1.6}\\ & =2.4\times {10}^5(8{)}^{\frac{5}{3}}=7.68\times {10}^6\mathrm{N}{\mathrm{m}}^{-2}\end{array}$

Work done in adiabatic process,

$\begin{array}{rl}& W=-\frac{P_2{V}_2-P_1{V}_1}{\gamma -1}\\ & =-\frac{(7.68\times {10}^6\times 0.875)-(2.4\times {10}^5\times 7)}{1.67-1}\\ & =-75.22\times {10}^5\mathrm{J}\end{array}$

Work done in the isothermal process,

$\begin{array}{rl}& W=2.3026\mathrm{RT}\log \frac{V_2}{V_1}=2.3026P_1{V}_1\log \frac{V_2}{V_1}\\ & =2.3026\times 2.4\times {10}^5\times 7\times \log \left[\frac{0.875}{7.0}\right]\\ & =2.3026\times 2.4\times {10}^5\times 7\log \left(\frac{1}{8}\right)=-34\times {10}^5\mathrm{J}\end{array}$

Difference in work done $=-75.22\times {10}^5\mathrm{J}+34\times {10}^5\mathrm{J}=-41.22\times {10}^5\mathrm{J}$

Q.4 1 mole of helium expands with temperature according to the relation $V=K{T}^{2/3}$. If the temperature changes by 60 K, find the heat absorbed (in J) by the monoatomic gas in the above process.

a) 1080.30
b) 1120.32
c) 1200
d) 1150.20

Answer:

$\begin{array}{rl}& V=K{T}^{2/3}\\ \Rightarrow & V=K{\left(\frac{PV}{nR}\right)}^{2/3}\\ \Rightarrow & P{V}^{-1/2}=\alpha \\ \because & C=C_V+\frac{R}{1-x}=\frac{3R}{2}+\frac{R}{1+\frac{1}{2}}=\frac{13R}{6}\\ Q& =nC\mathrm{\Delta }T=1\times \frac{13R}{6}\times 60=130R=1080.30\mathrm{J}\end{array}$

Hence, the answer is the option (a).

Q.5. A diatomic ideal gas is heated at constant volume until the pressure is doubled and again heated at constant pressure until volume is doubled. The average molar heat capacity for the whole process is $\frac{a}{b}R$. Find the remainder when $a$ is divided by $b$

Answer:

Let initial pressure, volume and temperature be $P_0,V_0,T_0$ indicated by state A in the P-V diagram. The gas is isochorically taken to state $B(2P_0,V_0,2T_0)$ and then taken from state B to state $\mathrm{C}(2P_0,2V_0,4T_0)$ isobarically.

Total heat absorbed by 1 mole of gas

$\begin{array}{rl}& \mathrm{\Delta }Q=C_v(2T_0-T_0)+C_P(4T_0-2T_0)\\ & =\frac{5}{2}R{T}_0+\frac{7}{2}R\times 2T_0\\ & =\frac{19}{2}R{T}_0\end{array}$
Total change in temperature from state A to C is: $\mathrm{\Delta }T=3T_0$
$\therefore$ Molar heat capacity $=\frac{\mathrm{\Delta }Q}{\mathrm{\Delta }T}=\frac{\frac{19}{2}R{T}_0}{3T_0}=\frac{19}{6}R$

Hence, the answer is 1.