Q. 134. Find the entropy increment of v = 2.0 moles of an ideal gas whose adiabatic exponent γ = 1.30 if, as a result of a certain process, the gas volume increased α = 2.0 times while the pressure dropped β = 3.0 times.
Solution. 134.
The entropy change depends on the initial and final state only so can be calculated for any process whatsoever.
We choose to evaluate the entropy change along the pair of lines shown above. Then
Q. 135. Vessels 1 and 2 contain v = 1.2 moles of gaseous helium. The ratio of the vessels' volumes V_{2}/V_{1} = α = 2.0, and the ratio of the absolute temperatures of helium in them T_{1}/T_{2} = β = 1.5. Assuming the gas to be ideal, find the difference of gas entropies in these vessels, S_{2}  S_{1}.
Solution. 135. To calculate the required entropy difference we only have to calculate the entropy difference for a process in which the state of the gas in vessel 1 is changed to that in vessel 2.
Q. 136. One mole of an ideal gas with the adiabatic exponent y goes through a polytropic process as a result of which the absolute temperature of the gas increases τfold. The polytropic constant equals n. Find the entropy increment of the gas in this process.
Solution. 136. For the polytropic process with index n
pV^{n} = constant
So
Q. 137. The expansion process of v = 2.0 moles of argon proceeds so that the gas pressure increases in direct proportion to its volume. Find the entropy increment of the gas in this process provided its volume increases α = 2.0 times.
Solution. 137. The process in question may be written as
where a is a constant and p_{0}, V_{0} are some reference values.
Along the line volume increases α times then so does the pressure. The temperature must then increase α^{2} times. Thus
if
Q. 138. An ideal gas with the adiabatic exponent γ goes through a process p = p_{0} — αV, where p_{0} and α are positive constants, and V is the volume. At what volume will the gas entropy have the maximum value?
Solution. 138. Let (p_{1}, V_{1}) be a reference point on the line
p = P_{0}  αV
and le t (p, V) be any other point.
The entropy difference
This gives a maximum of
(Note : a maximum of ΔS is a maximum of S (p, V))
Q. 139. One mole of an ideal gas goes through a process in which the entropy of the gas changes with temperature T as S = aT + C_{v} In T, where a is a positive constant, C_{v} is the molar heat capacity of this gas at constant volume. Find the volume dependence of the gas temperature in this process if T = T_{0} at V = V_{0}.
Solution. 139. Along the process line : S = aT + C_{y}In T
or the specific heat is :
O n the other hand : : dQ = CdT = C_{v}dT+pdV for an ideal gas.
Thus,
or
Using
Q. 140. Find the entropy increment of one mole of a Van der Waals gas due to the isothermal variation of volume from V_{1} to V_{2}. The Van der Waals corrections are assumed to be known.
Solution. 140. For a Vander Waal gas
The entropy change along an isotherm can be calculated from
It follows from (Q.129) that
assuming a, b to be known constants.
Thus
Q. 141. One mole of a Van der Waals gas which had initially the volume V_{1} and the temperature T_{1} was transferred to the state with the volume V_{2} and the temperature T_{2}. Find the corresponding entropy increment of the gas, assuming its molar heat capacity C_{v} to be known.
Solution. 141.
assuming C_{v} , a, b to be known constants.
Q. 142. At very low temperatures the heat capacity of crystals is equal to C = aT^{3}, where a is a constant. Find the entropy of a crystal as a function of temperature in this temperature interval.
Solution. 142. We can take 5 → 0 as T → 0 Then
Q. 143. Find the entropy increment of an aluminum bar of mass m = 3.0 kg on its heating from the temperature T_{1} = 300 K up to T_{2} = 600 K if in this temperature interval the specific heat capacity of aluminum varies as c = a + bT, where a = 0.77 J/(g• K), b = 0.46 mJ/(g• K^{2}).
Solution. 143.
Q. 144. In some process the temperature of a substance depends on its entropy S as T = aS^{n}, where a and n are constants. Find the corresponding heat capacity C of the substance as a function of S. At what condition is C < 0?
Solution. 144.
Then
Clearly C < 0 if n < 0.
Q. 145. Find the temperature T as a function of the entropy S of a substance for a polytropic process in which the heat capacity of the substance equals C. The entropy of the substance is known to be equal to S_{0} at the temperature T_{0}. Draw the approximate plots T (S) for C > 0 and C < 0.
Solution. 145.
We know,
assuming C to be a known constant.
Q. 146. One mole of an ideal gas with heat capacity C_{v} goes through a process in which its entropy S depends on T as S = α/T, where a is a constant. The gas temperature varies from T_{1} to T_{2}. Find:
(a) the molar heat capacity of the gas as a function of its temperature;
(b) the amount of heat transferred to the gas;
(c) the work performed by the gas.
Solution. 146.
Since for an ideal gas C_{v} is constant and ΔU = C_{V}(T_{2} T_{1})
Q. 147. A working substance goes through a cycle within which the absolute temperature varies nfold, and the shape of the cycle is shown in (a) Fig. 2.4a; (b) Fig. 2.4b, where T is the absolute temperature, and S the entropy. Find the efficiency of each cycle.
Solution. 147.
(a) We have from the definition
Q. 148. One of the two thermally insulated vessels interconnected by a tube with a valve contains v = 2.2 moles of an ideal gas. The other vessel is evacuated. The valve having been opened, the gas increased its volume n = 3.0 times. Find the entropy increment of the gas.
Solution. 148. In this case, called free expansion no work is done and no heat is exchanged. So internal eneigy must remain unchanged U_{f} = U_{i} For an ideal gas this implies constant temperature T_{f} = T_{i}. The process is irreversible but the entropy change can be calculated by considering a reversible isothermal process. Then, as before
Q. 149. A weightless piston divides a thermally insulated cylinder into two equal parts. One part contains one mole of an ideal gas with adiabatic exponent γ, the other is evacuated. The initial gas temperature is T_{0}. The piston is released and the gas fills the whole volume of the cylinder. Then the piston is slowly displaced back to the initial position. Find the increment of the internal energy and the entropy of the gas resulting from these two processes.
Solution. 149. The process consists of two parts. The first part is free expansion in which U_{f} = U_{i}. The second part is adiabatic compression in which work done results in change of internal energy. Obviously,
Now in the first part because there is no change of temperature.
In the second part,
Thus
The entropy change
as the process is reversible adiabatic. Thus ΔS = R In 2.
Q. 150. An ideal gas was expanded from the initial state to the volume V without any heat exchange with the surrounding bodies. Will the final gas pressure be the same in the case of (a) a fast and in the case of (b) a very slow expansion process?
Solution. 150. In all adiabatic processes
by virtue of the first law of thermodynamics. Thus,
For a slow process, where for a quasistatic adiabatic process
On the other hand for a fast process the external work done is for free expansion.
Since U depends on temperature only,
Consequently,
(From the ideal gas equation pV = RT)
Q. 151. A thermally insulated vessel is partitioned into two parts so that the volume of one part is n = 2.0 times greater than that of the other. The smaller part contains v_{1} = 0.30 mole of nitrogen, and the greater one v_{2} = 0.70 mole of oxygen. The temperature of the gases is the same. A hole is punctured in the partition and the gases are mixed. Find the corresponding increment of the system's entropy, assuming the gases to be ideal.
Solution. 151.
Since the temperature is the same, the required entropy change can be calculated by considering isothermal expansion of the gas in either parts into the whole vessel.
Thus
Q. 152. A piece of copper of mass m_{1} = 300 g with initial temperature t_{1} = 97°C is placed into a calorimeter in which the water of mass m_{2} = 100 g is at a temperature t_{2} = 7°C. Find the entropy increment of the system by the moment the temperatures equalize. The heat capacity of the calorimeter itself is negligibly small.
Solution. 152. Let c_{1} = specific heat of copper specific heat of water = c_{2}
T_{0} is found from
using
Q. 153. Two identical thermally insulated vessels interconnected by a tube with a valve contain one mole of the same ideal gas each. The gas temperature in one vessel is equal to T_{1} and in the other, T_{2}. The molar heat capacity of the gas of constant volume equals C_{v}. The valve having been opened, the gas comes to a new equilibrium state. Find the entropy increment ΔS of the gas. Demonstrate that ΔS > 0.
Solution. 153. For an ideal gas the internal energy depends on temperature only. We can consider the process in question to be one of simultaneous free expansion. Then the total energy U = U_{1} + U_{2}. Since
is the final temperature. The entropy change is obtained by considering isochoric processes because in effect, the gas remains confined to its vessel.
Since
Q. 154. N atoms of gaseous helium are enclosed in a cubic vessel of volume 1.0 cm3 at room temperature. Find:
(a) the probability of atoms gathering in one half of the vessel;
(b) the approximate numerical value of N ensuring the occurrence of this event within the time interval years (the age of the Universe).
of this event within the time interval t 101° years (the age of the Universe).
Solution. 154. (a) Each atom has a probability 1/2 to be in either campartment Thus
p = 2^{N}
(b) Typical atomic velocity at room temperature is cm/s so it takes an atom 10^{5} sec to cross the vessel. This is the relevant time scale for our problem. Let T = 10^{5} sec, then in time t there will be t/ T crossing or arrangements of the atoms. Ttys will be large enough to produce the given arrangement if
Q. 155. Find the statistical weight of the most probable distribution of N = 10 identical molecules over two halves of the cylinder's volume. Find also the probability of such a distribution.
Solution. 155. The statistical weight is
The probability distribution is
Q. 156. A vessel contains N molecules of an ideal gas. Dividing mentally the vessel into two halves A and B, find the probability that the half A contains n molecules. Consider the cases when N = 5 and n = 0, 1, 2, 3, 4, 5.
Solution. 156. The probabilites that the Jia lf A contains n molecules is
Q. 157. A vessel of volume V_{0} contains N molecules of an ideal gas. Find the probability of n molecules getting into a certain separated part of the vessel of volume V. Examine, in particular, the case V = V_{0}/2.
Solution. 157. The probability of one molecule being confined to the marked volume is
We can choose this molecule in many ways. The probability that n molecules get confined to the marked volume is cearly
Q. 158. An ideal gas is under standard conditions. Find the diameter of the sphere within whose volume the relative fluctuation of the number of molecules is equal to η = 1.0.10^{3}. What is the average number of molecules inside such a sphere?
Solution. 158. In a sphere of diameter d there are
where n_{0} = Loschmidt’s number = No. of molecules per unit volume (1 cc) under NTP. The relative fluctuation in this number is
The average number of molecules in this sphere is
Q. 159. One mole of an ideal gas consisting of monatomic molecules is enclosed in a vessel at a temperature T_{0} = 300 K. How many times and in what way will the statistical weight of this system (gas) vary if it is heated isochorically by ΔT = 1.0 K?
Solution. 159. For a monoatomic gas
The entropy change in the process is
Now from the Boltzmann equation
S = k lnΩ
Thus the statistical weight increases by this factor.
1. What is the second law of thermodynamics? 
2. How is entropy related to the second law of thermodynamics? 
3. Can you explain the concept of entropy in thermodynamics? 
4. What are the practical implications of the second law of thermodynamics? 
5. How does the second law of thermodynamics relate to realworld applications? 

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