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Page 1
Introductory Exercise 18.2
Q 1. One mole of an ideal mono atomic gas is initially at 300 K. Find the final temperature if 200 J of
heat are added as follows:
(a) at constant volume (b) at constant pressure.
Q 2. Prove that work done by an ideal gas in an adiabatic process is
i i f f
PV P V
W
1
?
?
??
, using the
integration PdV
?
.
Q 3. When a gas expands along AB it does 500 J of work and absorbs 250 J of heat. When the gas
expands along AC, it does 700 J of work and absorbs 300 J of heat.
(a) How much heat does the gas exchange along BC?
(b) When the gas makes the transition from C to A along CDA, 800 J of work are done on it from
C to D. How much heat does it exchange along CDA ?
Q 4. One mole of an ideal monoatomic gas occupies a volume of 1.0 × 10
-2
m
3
at a pressure of
2.0 × 10
5
N/m
2
.
(a) What is the temperature of the gas?
(b) The gas undergoes an adiabatic compression until its volume is decreased to 5.0 × 10
-3
m
3
.
What is the new gas temperature?
(c) How much work is done on the gas during the compression?
(d) What is the change in the internal energy of the gas?
Q 5. A bullet of mass 10 g travelling horizontally at 200 m/s strikes and embeds in a pendulum bob of
mass 2.0 kg.
(a) How much mechanical energy is dissipated in the collision?
(b) Assuming that C
v
for the bob plus bullet is 3 R, calculate the temperature increase of the
system due to the collision. Take the molecular mass of the system to be 200 g/mol.
Q 6. An ideal gas is carried through a thermodynamic cycle consisting of two isobaric and two
isothermal processes, as shown in figure. Show that the net work done in the entire cycle is given
by the equation.
Q 7. Consider the cyclic process depicted in figure. If Q is negative for the process BC, and if. ?U is
negative for the process CA, what are the signs of Q, W and ?U that are associated with each
process?
Page 2
Introductory Exercise 18.2
Q 1. One mole of an ideal mono atomic gas is initially at 300 K. Find the final temperature if 200 J of
heat are added as follows:
(a) at constant volume (b) at constant pressure.
Q 2. Prove that work done by an ideal gas in an adiabatic process is
i i f f
PV P V
W
1
?
?
??
, using the
integration PdV
?
.
Q 3. When a gas expands along AB it does 500 J of work and absorbs 250 J of heat. When the gas
expands along AC, it does 700 J of work and absorbs 300 J of heat.
(a) How much heat does the gas exchange along BC?
(b) When the gas makes the transition from C to A along CDA, 800 J of work are done on it from
C to D. How much heat does it exchange along CDA ?
Q 4. One mole of an ideal monoatomic gas occupies a volume of 1.0 × 10
-2
m
3
at a pressure of
2.0 × 10
5
N/m
2
.
(a) What is the temperature of the gas?
(b) The gas undergoes an adiabatic compression until its volume is decreased to 5.0 × 10
-3
m
3
.
What is the new gas temperature?
(c) How much work is done on the gas during the compression?
(d) What is the change in the internal energy of the gas?
Q 5. A bullet of mass 10 g travelling horizontally at 200 m/s strikes and embeds in a pendulum bob of
mass 2.0 kg.
(a) How much mechanical energy is dissipated in the collision?
(b) Assuming that C
v
for the bob plus bullet is 3 R, calculate the temperature increase of the
system due to the collision. Take the molecular mass of the system to be 200 g/mol.
Q 6. An ideal gas is carried through a thermodynamic cycle consisting of two isobaric and two
isothermal processes, as shown in figure. Show that the net work done in the entire cycle is given
by the equation.
Q 7. Consider the cyclic process depicted in figure. If Q is negative for the process BC, and if. ?U is
negative for the process CA, what are the signs of Q, W and ?U that are associated with each
process?
Q 8. An ideal gas is enclosed in a cylinder with a movable piston on top. The piston has mass of 8000 g
and an area of 5.00 cm
2
and is free to slide up and down, keeping the pressure of the gas constant.
How much work is done as the temperature of 0.200 mol of the gas is raised from 200°C to
300°C?
Q 9. A sample of ideal gas is expanded to twice its original volume of 1.00 m
3
in a quasi-static process
for which P = ?V
2
, with
?
= 5.00 atm/m
6
, as shown in figure. How much work is done by the
expanding gas?
Solutions
1. (a)
or 200 = 1.5 × 8.31(T
f
-300)
Solving we get, T
f
= 316 K
(b)
or 200 = 2.5 × 8.31(T
f
-300)
Solving we get, T
f
= 309.6 K
2. In adiabatic process,
PV
?
= constant = K (say)
Page 3
Introductory Exercise 18.2
Q 1. One mole of an ideal mono atomic gas is initially at 300 K. Find the final temperature if 200 J of
heat are added as follows:
(a) at constant volume (b) at constant pressure.
Q 2. Prove that work done by an ideal gas in an adiabatic process is
i i f f
PV P V
W
1
?
?
??
, using the
integration PdV
?
.
Q 3. When a gas expands along AB it does 500 J of work and absorbs 250 J of heat. When the gas
expands along AC, it does 700 J of work and absorbs 300 J of heat.
(a) How much heat does the gas exchange along BC?
(b) When the gas makes the transition from C to A along CDA, 800 J of work are done on it from
C to D. How much heat does it exchange along CDA ?
Q 4. One mole of an ideal monoatomic gas occupies a volume of 1.0 × 10
-2
m
3
at a pressure of
2.0 × 10
5
N/m
2
.
(a) What is the temperature of the gas?
(b) The gas undergoes an adiabatic compression until its volume is decreased to 5.0 × 10
-3
m
3
.
What is the new gas temperature?
(c) How much work is done on the gas during the compression?
(d) What is the change in the internal energy of the gas?
Q 5. A bullet of mass 10 g travelling horizontally at 200 m/s strikes and embeds in a pendulum bob of
mass 2.0 kg.
(a) How much mechanical energy is dissipated in the collision?
(b) Assuming that C
v
for the bob plus bullet is 3 R, calculate the temperature increase of the
system due to the collision. Take the molecular mass of the system to be 200 g/mol.
Q 6. An ideal gas is carried through a thermodynamic cycle consisting of two isobaric and two
isothermal processes, as shown in figure. Show that the net work done in the entire cycle is given
by the equation.
Q 7. Consider the cyclic process depicted in figure. If Q is negative for the process BC, and if. ?U is
negative for the process CA, what are the signs of Q, W and ?U that are associated with each
process?
Q 8. An ideal gas is enclosed in a cylinder with a movable piston on top. The piston has mass of 8000 g
and an area of 5.00 cm
2
and is free to slide up and down, keeping the pressure of the gas constant.
How much work is done as the temperature of 0.200 mol of the gas is raised from 200°C to
300°C?
Q 9. A sample of ideal gas is expanded to twice its original volume of 1.00 m
3
in a quasi-static process
for which P = ?V
2
, with
?
= 5.00 atm/m
6
, as shown in figure. How much work is done by the
expanding gas?
Solutions
1. (a)
or 200 = 1.5 × 8.31(T
f
-300)
Solving we get, T
f
= 316 K
(b)
or 200 = 2.5 × 8.31(T
f
-300)
Solving we get, T
f
= 309.6 K
2. In adiabatic process,
PV
?
= constant = K (say)
3. (a) U
C
- U
A
along two paths should be same.
(Q
AB
+ Q
BC
) - (W
AB
+ W
BC
) = Q
AC
- W
AC
? (250 + Q
BC
) - (500 + 0) = 300 - 700 Solving we get
Q
BC
= -150 J
(b) Q
CDA
= W
CD
+ W
DA
)+ (U
A
- U
C
)
= (-800+ 0) - (U
C
- U
A
)
= - 800 - (300 - 700) = - 400 J
4. (a)
(b) In adiabatic process
(c) Work done on the gas = ?U
= 1.5 × 8.31(383-240.7) ? 1770 J
(d) ?U ? 1770 J
5. (a) From conservation of linear momentum
0.01 × 200 = (2+0.01) v
V ? 1 m/s
Mechanical energy dissipated in collision = K
i
- K
f
? 199 J
(b)
Using,
Q = nC
V
?T
= 0.80°C
6. Along the process CD apply,
PV - constant and find V
C
Similarly along path AB, again apply,
PV = constant and find Y
B
Now, W
nett
= W
AB
+ W
BC
+ W
CD
+ W
DA
Page 4
Introductory Exercise 18.2
Q 1. One mole of an ideal mono atomic gas is initially at 300 K. Find the final temperature if 200 J of
heat are added as follows:
(a) at constant volume (b) at constant pressure.
Q 2. Prove that work done by an ideal gas in an adiabatic process is
i i f f
PV P V
W
1
?
?
??
, using the
integration PdV
?
.
Q 3. When a gas expands along AB it does 500 J of work and absorbs 250 J of heat. When the gas
expands along AC, it does 700 J of work and absorbs 300 J of heat.
(a) How much heat does the gas exchange along BC?
(b) When the gas makes the transition from C to A along CDA, 800 J of work are done on it from
C to D. How much heat does it exchange along CDA ?
Q 4. One mole of an ideal monoatomic gas occupies a volume of 1.0 × 10
-2
m
3
at a pressure of
2.0 × 10
5
N/m
2
.
(a) What is the temperature of the gas?
(b) The gas undergoes an adiabatic compression until its volume is decreased to 5.0 × 10
-3
m
3
.
What is the new gas temperature?
(c) How much work is done on the gas during the compression?
(d) What is the change in the internal energy of the gas?
Q 5. A bullet of mass 10 g travelling horizontally at 200 m/s strikes and embeds in a pendulum bob of
mass 2.0 kg.
(a) How much mechanical energy is dissipated in the collision?
(b) Assuming that C
v
for the bob plus bullet is 3 R, calculate the temperature increase of the
system due to the collision. Take the molecular mass of the system to be 200 g/mol.
Q 6. An ideal gas is carried through a thermodynamic cycle consisting of two isobaric and two
isothermal processes, as shown in figure. Show that the net work done in the entire cycle is given
by the equation.
Q 7. Consider the cyclic process depicted in figure. If Q is negative for the process BC, and if. ?U is
negative for the process CA, what are the signs of Q, W and ?U that are associated with each
process?
Q 8. An ideal gas is enclosed in a cylinder with a movable piston on top. The piston has mass of 8000 g
and an area of 5.00 cm
2
and is free to slide up and down, keeping the pressure of the gas constant.
How much work is done as the temperature of 0.200 mol of the gas is raised from 200°C to
300°C?
Q 9. A sample of ideal gas is expanded to twice its original volume of 1.00 m
3
in a quasi-static process
for which P = ?V
2
, with
?
= 5.00 atm/m
6
, as shown in figure. How much work is done by the
expanding gas?
Solutions
1. (a)
or 200 = 1.5 × 8.31(T
f
-300)
Solving we get, T
f
= 316 K
(b)
or 200 = 2.5 × 8.31(T
f
-300)
Solving we get, T
f
= 309.6 K
2. In adiabatic process,
PV
?
= constant = K (say)
3. (a) U
C
- U
A
along two paths should be same.
(Q
AB
+ Q
BC
) - (W
AB
+ W
BC
) = Q
AC
- W
AC
? (250 + Q
BC
) - (500 + 0) = 300 - 700 Solving we get
Q
BC
= -150 J
(b) Q
CDA
= W
CD
+ W
DA
)+ (U
A
- U
C
)
= (-800+ 0) - (U
C
- U
A
)
= - 800 - (300 - 700) = - 400 J
4. (a)
(b) In adiabatic process
(c) Work done on the gas = ?U
= 1.5 × 8.31(383-240.7) ? 1770 J
(d) ?U ? 1770 J
5. (a) From conservation of linear momentum
0.01 × 200 = (2+0.01) v
V ? 1 m/s
Mechanical energy dissipated in collision = K
i
- K
f
? 199 J
(b)
Using,
Q = nC
V
?T
= 0.80°C
6. Along the process CD apply,
PV - constant and find V
C
Similarly along path AB, again apply,
PV = constant and find Y
B
Now, W
nett
= W
AB
+ W
BC
+ W
CD
+ W
DA
Further, nRT
A
=P
A
V
A
and nRT
C
= P
C
V
C
7. AB
V is increasing, so W = + ve. Product of PV and therefore T and therefore U is increasing.
So, ?U
is also +ve
Q = W + ?V
? Q is also positive.
EC
V = constant
? W = 0
Q = ?U = - ve
CA
V is decreasing.
? W =-ve
?U
is also negative.
? Q = W + ?U is also negative.
8. PV = nRT
? P ?V = nR ?T
Work done under constant pressure is,
W = P ?V = nR ?T
= (0.2)(8.31)(100)= 166.2 J
9.
Solving we get, W = 1.18 × 10
6
J
= 1.18 MJ
Introductory Exercise 18.3
Q 1. Three moles of an ideal gas being initially at a temperature T
i
= 273 K were isothermally
expanded 5 times its initial volume and then isochorically heated so that the pressure in the final
state become equal to that in the initial state. The total heat supplied in the process is 80 kJ. Find
P
V
C
C
??
??
??
??
of the gas.
Q 2. As a result of the isobaric heating by ?T = 72 K, one mole of a certain ideal gas obtains an amount
of heat Q =1.6 kJ. Find the work performed by the gas, the increment of its internal energy and ?.
Q 3. A gas undergoes the cycle shown in figure. The cycle is repeated 100 times per minute. Determine
the power generated.
Page 5
Introductory Exercise 18.2
Q 1. One mole of an ideal mono atomic gas is initially at 300 K. Find the final temperature if 200 J of
heat are added as follows:
(a) at constant volume (b) at constant pressure.
Q 2. Prove that work done by an ideal gas in an adiabatic process is
i i f f
PV P V
W
1
?
?
??
, using the
integration PdV
?
.
Q 3. When a gas expands along AB it does 500 J of work and absorbs 250 J of heat. When the gas
expands along AC, it does 700 J of work and absorbs 300 J of heat.
(a) How much heat does the gas exchange along BC?
(b) When the gas makes the transition from C to A along CDA, 800 J of work are done on it from
C to D. How much heat does it exchange along CDA ?
Q 4. One mole of an ideal monoatomic gas occupies a volume of 1.0 × 10
-2
m
3
at a pressure of
2.0 × 10
5
N/m
2
.
(a) What is the temperature of the gas?
(b) The gas undergoes an adiabatic compression until its volume is decreased to 5.0 × 10
-3
m
3
.
What is the new gas temperature?
(c) How much work is done on the gas during the compression?
(d) What is the change in the internal energy of the gas?
Q 5. A bullet of mass 10 g travelling horizontally at 200 m/s strikes and embeds in a pendulum bob of
mass 2.0 kg.
(a) How much mechanical energy is dissipated in the collision?
(b) Assuming that C
v
for the bob plus bullet is 3 R, calculate the temperature increase of the
system due to the collision. Take the molecular mass of the system to be 200 g/mol.
Q 6. An ideal gas is carried through a thermodynamic cycle consisting of two isobaric and two
isothermal processes, as shown in figure. Show that the net work done in the entire cycle is given
by the equation.
Q 7. Consider the cyclic process depicted in figure. If Q is negative for the process BC, and if. ?U is
negative for the process CA, what are the signs of Q, W and ?U that are associated with each
process?
Q 8. An ideal gas is enclosed in a cylinder with a movable piston on top. The piston has mass of 8000 g
and an area of 5.00 cm
2
and is free to slide up and down, keeping the pressure of the gas constant.
How much work is done as the temperature of 0.200 mol of the gas is raised from 200°C to
300°C?
Q 9. A sample of ideal gas is expanded to twice its original volume of 1.00 m
3
in a quasi-static process
for which P = ?V
2
, with
?
= 5.00 atm/m
6
, as shown in figure. How much work is done by the
expanding gas?
Solutions
1. (a)
or 200 = 1.5 × 8.31(T
f
-300)
Solving we get, T
f
= 316 K
(b)
or 200 = 2.5 × 8.31(T
f
-300)
Solving we get, T
f
= 309.6 K
2. In adiabatic process,
PV
?
= constant = K (say)
3. (a) U
C
- U
A
along two paths should be same.
(Q
AB
+ Q
BC
) - (W
AB
+ W
BC
) = Q
AC
- W
AC
? (250 + Q
BC
) - (500 + 0) = 300 - 700 Solving we get
Q
BC
= -150 J
(b) Q
CDA
= W
CD
+ W
DA
)+ (U
A
- U
C
)
= (-800+ 0) - (U
C
- U
A
)
= - 800 - (300 - 700) = - 400 J
4. (a)
(b) In adiabatic process
(c) Work done on the gas = ?U
= 1.5 × 8.31(383-240.7) ? 1770 J
(d) ?U ? 1770 J
5. (a) From conservation of linear momentum
0.01 × 200 = (2+0.01) v
V ? 1 m/s
Mechanical energy dissipated in collision = K
i
- K
f
? 199 J
(b)
Using,
Q = nC
V
?T
= 0.80°C
6. Along the process CD apply,
PV - constant and find V
C
Similarly along path AB, again apply,
PV = constant and find Y
B
Now, W
nett
= W
AB
+ W
BC
+ W
CD
+ W
DA
Further, nRT
A
=P
A
V
A
and nRT
C
= P
C
V
C
7. AB
V is increasing, so W = + ve. Product of PV and therefore T and therefore U is increasing.
So, ?U
is also +ve
Q = W + ?V
? Q is also positive.
EC
V = constant
? W = 0
Q = ?U = - ve
CA
V is decreasing.
? W =-ve
?U
is also negative.
? Q = W + ?U is also negative.
8. PV = nRT
? P ?V = nR ?T
Work done under constant pressure is,
W = P ?V = nR ?T
= (0.2)(8.31)(100)= 166.2 J
9.
Solving we get, W = 1.18 × 10
6
J
= 1.18 MJ
Introductory Exercise 18.3
Q 1. Three moles of an ideal gas being initially at a temperature T
i
= 273 K were isothermally
expanded 5 times its initial volume and then isochorically heated so that the pressure in the final
state become equal to that in the initial state. The total heat supplied in the process is 80 kJ. Find
P
V
C
C
??
??
??
??
of the gas.
Q 2. As a result of the isobaric heating by ?T = 72 K, one mole of a certain ideal gas obtains an amount
of heat Q =1.6 kJ. Find the work performed by the gas, the increment of its internal energy and ?.
Q 3. A gas undergoes the cycle shown in figure. The cycle is repeated 100 times per minute. Determine
the power generated.
Solutions
1. First process
T = constant
V is made 5 times. Therefore P will become
1
th
5
.
Second process
V = constant
Pressure again becomes first times. So, temperature will also become 5 times.
Q
1
+ Q
2
= 80 × 10
3
= 80 × l0
3
Solving we get, ?
= 1.4
2. W = nR ?T (in isobaric process)
= (1) (8.31)(72) = 600 J = 0.6 kJ
3. Work done per cycle = area under the cycle
= 1010 J
Total work done per second
= 1683 J/s = 1.68 W
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FAQs on DC Pandey Solutions: First Law of Thermodynamics - 2 - Physics Class 11 - NEET
| 1. What is the first law of thermodynamics? |  |
Ans. The first law of thermodynamics, also known as the law of energy conservation, states that energy cannot be created or destroyed in an isolated system. It can only be transferred or converted from one form to another.
| 2. How is the first law of thermodynamics applied in real-life situations? | |
Ans. The first law of thermodynamics finds applications in various real-life situations. For example, it helps in understanding the energy transfer and conversion processes in engines, such as car engines or power plant turbines. It also helps in analyzing the energy flow in heating and cooling systems, as well as studying the behavior of gases and fluids in different processes.
| 3. What are the implications of the first law of thermodynamics for energy efficiency? | |
Ans. The first law of thermodynamics implies that the total energy input to a system is equal to the total energy output, considering all the energy transfers and conversions. This has implications for energy efficiency, as it indicates that minimizing energy losses during these processes is crucial for achieving high efficiency. By understanding and applying the first law, engineers and scientists can develop more efficient systems and technologies.
| 4. Can the first law of thermodynamics be violated? | |
Ans. The first law of thermodynamics is a fundamental principle of nature and is believed to hold true in all situations. It has been extensively tested and verified through various experiments and observations. Hence, it is considered a law of nature, and violating it would mean going against the established scientific understanding.
| 5. How is the first law of thermodynamics related to the concept of internal energy? | |
Ans. The first law of thermodynamics is closely related to the concept of internal energy. Internal energy is the sum of all the microscopic energies within a system, including the kinetic and potential energies of its particles. According to the first law, the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. This relationship allows us to analyze and understand the energy changes within a system based on the first law of thermodynamics.
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DC Pandey Solutions: First Law of Thermodynamics - 2 NEET Questions
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