Irodov Solutions: The First Law of Thermodynamics, Heat Capacity | Physics Class 11 - NEET PDF Download

Q1: Demonstrate that the internal energy U of the air in a room is independent of temperature provided the outside pressure p is constant. Calculate U, if p is equal to the normal atmospheric pressure and the room's volume is equal to V = 40 m³. 

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Ans: Internal energy of air, treating as an ideal gas

   (1)

Using  

Thus at constant pressure U = constant, because the volume of the room is a constant.

Putting the value of p = P_atm and V in Eq. (1), we get U = 10 MJ.

Q2: A thermally insulated vessel containing a gas whose molar mass is equal to M and the ratio of specific heats Cp/Cv  = γ  moves with a velocity v. Find the gas temperature increment resulting from the sudden stoppage of the vessel. 

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Ans: From energy conservation

or,           (1)

But from    (from the previous problem)     (2)

Hence from Eqs. (1) and (2).

Q3: Two thermally insulated vessels 1 and 2 are filled with air and connected by a short tube equipped with a valve. The volumes of the vessels, the pressures and temperatures of air in them are known (V₁, p₁, T₁ and V₂, p₂, T₂). Find the air temperature and pressure established after the opening of the valve. 

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Ans: On opening the valve, the air will flow from the vessel at higher pressure to the vessel at lower pressure till both vessels have the same air pressure. If this air pressure is p, the total volume of the air in the two vessels will be (V₁ + V₂). Also if v₁ and v₂ be the number of moles of air initially in the two vessels, we have

    (1)

After the air is mixed up, the total number of moles are (v₁ + v₂) and the mixture is at temperature T.

Hence       (2)

Let us look at the two portions of air as one single system. Since this system is contained in a thermally insulated vessel, no heat exchange is involved in the process. That is, total heat transfer for the combined system Q = 0

Moreover, this combined system does not perform mechanical work either. The walls of the containers are rigid and there are no pistons etc. to be pushed, looking at the total system, we know A = 0.

Hence, internal energy of the combined system docs not change in the process. Initially energy of the combined system is equal to the sum of internal energies of the two portions of air :

     (3)

Final internal energy of (n₁ + n₂) moles of air at temperature T is given by

    (4)

Therefore, U_i = U_f implies :

From (2), therefore, final pressure is given by :

This process in an example of free adiabatic expansion of ideal gas.

Q4: Gaseous hydrogen contained initially under standard conditions in a sealed vessel of volume V = 5.0 l was cooled by ΔT = 55 K . Find how much the internal energy of the gas will change and what amount of heat will be lost by the gas.

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Ans: By the first law of thermodynamics,

Q = ΔU + A

Here A = 0, as the volume remains constant,

So,  

From gas law,  

Hence amount of heat lost  

Q5: What amount of heat is to be transferred to nitrogen in the isobaric heating process for that gas to perform the work A = 2.0 J? 

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Ans: By the first law of thermodynamics  Q = ΔU + A

But  

Q6: As a result of the isobaric heating by ΔT = 72 K one mole of a certain ideal gas obtains an amount of heat Q = 1.60 kJ. Find the work performed by the gas, the increment of its internal energy, and the value of γ = C_p/C_v.

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Ans: Under isobaric process

From the first law of thermodynamics 

Again increment in internal energy  

Thus  

Q7: Two moles of a certain ideal gas at a temperature T₀ = 300 K were cooled isochorically so that the gas pressure reduced n = 2.0 times. Then, as a result of the isobaric process, the gas expanded till its temperature got back to the initial value. Find the total amount of heat absorbed by the gas in this process. 

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Ans: Let v = 2 moles of the gas. In the first phase, under isochoric process, A₁ = 0, therefore from gas law if pressure is reduced n times so that temperature i.e. new temperature becomes T₀/n. 

Now from first law of thermodynamics

During the second phase (under isobaric process),

Thus from first law of thermodynamics :

Hence the total amount of heat absorbed

Q8: Calculate the value of γ = C_p/C_v  for a gaseous mixture consisting of v₁  = 2.0 moles of oxygen and v₂ = 3.0 moles of carbon dioxide. The gases are assumed to be ideal. 

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Ans: Total no. of moles of the mixture v = v₁ + v₂

At a certain temperature,  

Thus  

Similarly  

Thus  

Q9: Find the specific heat capacities c_v and c_p for a gaseous mixture consisting of 7.0 g of nitrogen and 20 g of argon. The gases are assumed to be ideal. 

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Ans: 

and    

Now molar mass of the mixture  

Hence  

Q10: One mole of a certain ideal gas is contained under a weightless piston of a vertical cylinder at a temperature T. The space over the piston opens into the atmosphere. What work has to be performed in order to increase isothermally the gas volume under the piston it times by slowly raising the piston? The friction of the piston against the cylinder walls is negligibly small. 

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Ans: Let 5 be the area of the piston and F be the force exerted by the external agent Then, F + p S - p₀S (Fig.) at an arbitrary instant of time. Here p is the pressure at the instant the volume is V. (Initially the pressure inside is p₀)

Q11: A piston can freely move inside a horizontal cylinder closed from both ends. Initially, the piston separates the inside space of the cylinder into two equal parts each of volume V₀, in which an ideal gas is contained under the same pressure P₀  and at the same temperature. What work has to be performed in order to increase isothermally the volume of one part of gas η times compared to that of the other by slowly moving the piston? 

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Ans: Let the agent move the piston to the right by x. In equilibrium position,

Work done by the agent in an infinitesmal change dx is

By applying PV = constant, for the two parts,

So,      

When the volume of the left end is η times the volume of the right end

Q12: Three moles of an ideal gas being initially at a temperature T₀ = 273 K were isothermally expanded n = 5.0 times its initial volume and then isochorically heated so that the pressure in the final state became 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 γ = C_p/C_v for this gas. 

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Ans: In the isothermal process, heat transfer to the gas is given by

In the isochoric process, A = 0

Thus heat transfer to the gas is given by

But  

or,  

Thus, net heat transfer to the gas

or,    

or,  

Q13: Draw the approximate plots of isochoric, isobaric, isothermal, and adiabatic processes for the case of an ideal gas, using the following variables:

(a) p, T; (b) V, T. 

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Ans: (a) From ideal gas law

For isochoric process, obviously k = constant, thus p = kT, represents a straight line passing through the origin and its slope becomes k.
For isobaric process p = constant, thus on p - T curve, it is a horizontal straight line parallel to T - axis, if T is along horizontal (or x - axis)

For isothermal process, T = constant, thus on p - T curve, it represents a vertical straight line if T is taken along horizontal (or x - axis)

For adiabatic process

After diffrentiating, we get

The approximate plots of isochoric, isobaric, isothermal, and adiabatic processes are drawn in the answer sheet.

(b) As p is not considered as variable, we have from ideal gas law

On V - T co-ordinate system let us, take T along x - axis.
For isochoric process V = constant, thus k' = constant and V = k'T obviously represents a straight line passing through the origin of the co-ordinate system and k' is its slope.
For isothermal process T = constant. Thus on the stated co- ordinate system it represents a straight line parallel to the V - axis.
For adiabatic process

After differentiating, we get

The approximate plots of isochoric, isobaric, isothermal and adiabatic processes are drawn in the answer sheet.

Q14: One mole of oxygen being initially at a temperature T₀ = 290 K is adiabatically compressed to increase its pressure η = 10.0 times. Find:
 (a) the gas temperature after the compression;
 (b) the work that has been performed on the gas. 

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Ans: According to T - p relation in adiabatic process,  (where k = constant)

and  

Hence  

(b) Using the solution of part (a), sought work done

Q15: A certain mass of nitrogen was compressed η = 5.0 times (in terms of volume), first adiabatically, and then isothermally. In both cases the initial state of the gas was the same. Find the ratio of the respective works expended in each compression.

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Ans: Let (p₀, V₀,T₀) be the initial state of the gas.

We know  

But from the equation  

Thus    

On the other hand, we know   (work done by the gas)

Thus  

Q16: A heat-conducting piston can freely move inside a closed thermally insulated cylinder with an ideal gas. In equilibrium the piston divides the cylinder into two equal parts, the gas temperature being equal to T₀ . The piston is slowly displaced. Find the gas temperature as a function of the ratio η of the volumes of the greater and smaller sections. The adiabatic exponent of the gas is equal to γ.

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Ans: Since here the piston is conducting and it is moved slowly the temperature on the two sides increases and maintained at the same value.
Elementary work done by the agent = Work done in compression - Work done in expansion 

i.e. dA - p₂ dV - p₁ dV = (p₂ - P₁) dV

where p₁ and p₂ are pressures at any instant of the gas on expansion and compression side respectively.

From the gas law   for each section

(x is the displacement of the piston towards section 2)

So,  

So  

Also, from the first law of thermodynamics 

So, work done on the gas  

On integrating 

or  

Hence  

Q17: Find the rate v with which helium flows out of a thermally insulated vessel into vacuum through a small hole. The flow rate of the gas inside the vessel is assumed to be negligible under these conditions. The temperature of helium in the vessel is T = 1,000 K.

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Ans: From energy conservation as in the derivation of Bernoulli theorem it reads

    (1)

In the Eq. (1) u is the internal energy per unit mass and in this case is the thermal eneigy per unit mass of the gas. As the gas vessel is thermally insulated Q_d = 0, also in our case.

Just inside the vessel  Inside the vessel v = 0 also. Just outside p = 0, and u = 0. Ingeneral gz is not very significant for gases.

Thus applying Eq. (1) just inside and outside the hole, we get

Hence  

Note : The velocity here is the velocity of hydrodynamic flow of the gas into vacuum. This requires that the diameter of the hole is not too small (D > mean free path l). In the opposite case (D < < l) the flow is called effusion. Then the above result does not apply and kinetic theory methods are needed.

Q18: The volume of one mole of an ideal gas with the adiabatic exponent γ is varied according to the law V = a/T, where a is a constant. Find the amount of heat obtained by the gas in this process if the gas temperature increased by ΔT. 

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Ans: The differential work done by the gas

So,  

From the Grst law of thermodynamics  

Q19: Demonstrate that the process in which the work performed by an ideal gas is proportional to the corresponding increment of its internal energy is described by the equation pVⁿ = const, where n is a constant. 

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Ans: According to the problem : A α U or dA = aU (where a is proportionality constant)

or,                                 (1)

From ideal gas law, pV= v R T, on differentiating

p dV + V dp = v RdT                      (2)

Thus from (1) and (2) 

or,  

Dividing both the sides by pV

On integrating n In V + In p = In C (where C is constant) 

or,

Q20: Find the molar heat capacity of an ideal gas in a polytropic process pVⁿ = const if the adiabatic exponent of the gas is equal to γ. At what values of the polytropic constant n will the heat capacity of the gas be negative? 

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Ans: In the polytropic process work done by the gas

(where T_i and T_f are initial and final temperature of the gas like in adiabatic process)

and    

By the first law of thermodynamics Q = ΔU + A 

According to definition of molar heat capacity when number of moles v = 1 and ΔT = 1 then Q = Molar heat capacity.

Here,    

Q21: In a certain polytropic process the volume of argon was increased α = 4.0 times. Simultaneously, the pressure decreased β = 8.0 times. Find the molar heat capacity of argon in this process, assuming the gas to be ideal.

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Ans: Let the process be polytropic according to the law pVⁿ = constant

Thus,  

So,  

In the polytropic process molar heat capacity is given by

So,  

Q22: One mole of argon is expanded polytropically, the polytropic constant being n = 1.50. In the process, the gas temperature changes by ΔT = — 26 K. Find:
 (a) the amount of heat obtained by the gas;
 (b) the work performed by the gas

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Ans: (a) Increment of internal energy for ΔT, becomes

From first law of thermodynamics

(b) Sought work done,  

 Q23: An ideal gas whose adiabatic exponent equals y is expanded according to the law p = αV , where a is a constant. The initial volume of the gas is equal to V₀. As a result of expansion the volume increases η times. Find:
 (a) the increment of the internal energy of the gas;
 (b) the work performed by the gas;
 (c) the molar heat capacity of the gas in the process.

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Ans: Law of the process is p = α V or pV^-1 = α
so the process is polytropic of index n = - 1
As p = αV so, P_i - αV₀ and p_f = α η V₀

(a) Increment of the internal energy is given by

(b) Work done by the gas is given by

(c) Molar heat capacity is given by

Q24: An ideal gas whose adiabatic exponent equals γ is expanded so that the amount of heat transferred to the gas is equal to the decrease of its internal energy. Find:
 (a) the molar heat capacity of the gas in this process;
 (b) the equation of the process in the variables T, V;
(c) the work performed by one mole of the gas when its volume increases η times if the initial temperature of the gas is T₀. 

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Ans:   

where C_n is the molar heat capacity in the process. It is given that

So,  

(b) By the first law of thermodynamics, dQ - dU + dA,

or,  

So,    

or,  

(c)  

But from part (a), we have  

Thus  

From part (b); we know  

So,  (where T is the final temperature)

Work done by the gas for one mole is given by

Q25: One mole of an ideal gas whose adiabatic exponent equals y undergoes a process in which the gas pressure relates to the temperature as p = aT^α, where a and α are constants. Find:
 (a) the work performed by the gas if its temperature gets an increment ΔT;
 (b) the molar heat capacity of the gas in this process; at what value of α will the heat capacity be negative? 

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Ans: Given p = a T^α (for one mole of gas)

So,  

or,  

Here polytropic exponent  

(a) In the poly tropic process for one mole of gas :

(b) Molar heat capacity is given by

Q26: An ideal gas with the adiabatic exponent γ undergoes a process in which its internal energy relates to the volume as U = aV^α, where a and α are constants. Find:
 (a) the work performed by the gas and the amount of heat to be transferred to this gas to increase its internal energy by ΔU;
 (b) the molar heat capacity of the gas in this process. 

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Ans: 

or,    

or,  

or  

So polytropric index n = 1 - α

(a) Work done by the gas is given by

Hence  

By the first law of thermodynamics, Q = ΔU+A

(b) Molar heat capacity is given by

Q27: An ideal gas has a molar heat capacity C_v at constant volume. Find the molar heat capacity of this gas as a function of its volume V, if the gas undergoes the following process: 

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Ans: By the first law .of thermodynamics

Molar specific heat according to definition

We have  

After differentiating, we get  

So,  

Hence  

(b)  

So,  

Q28: One mole of an ideal gas whose adiabatic exponent equals γ undergoes a process p = p₀ + α /V, w here P₀ and α are positive constants. Find:
 (a) heat capacity of the gas as a function of its volume;
(b) the internal energy increment of the gas, the work performed by it, and the amount of heat transferred to the gas, if its volume increased from V₁ to V₂.

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Ans: Using 2.52

 (for one mole of gas)

Therefore  

Hence  

(b) Work done is given by

By the first law of thermodynamics Q = ΔU +A

Q29: One mole of an ideal gas with heat capacity at constant pressure C_p undergoes the process T = T₀ + αV, where T₀ and α are constants. Find: 
 (a) heat capacity of the gas as a function of its volume;
(b) the amount of heat transferred to the gas, if its volume increased from V₁ to V₂. 

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Ans: (a) Heat capacity is given by

   (see solution of 2.52)

We have  

After differentiating, we get,  

Hence  

(b)  

 for one mole of gas

Now  

By the first law of thermodynamics Q = ΔU + A

Q30: For the case of an ideal gas find the equation of the process (in the variables T, V) in which the molar heat capacity varies as:
(a) C = C_v  + αT; (b) C = C_v + βV;  (c) C = C_v + ap, where α, β, and a are constants. 

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Ans: Heat capacity is given by

Integrating both sides, we get   is a constant.

Or,  

and  

or,  

Integrating both sides, we get  

So,  

So,  

or    

or,  

  or V - a T = constant

Q31: An ideal gas has an adiabatic exponent γ. In some process its molar heat capacity varies as C = α/T, where α is a constant. Find:
(a) the work performed by one mole of the gas during its heating from the temperature T₀ to the temperature η times higher; 
 (b) the equation of the process in the variables p, V. 

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Ans: (a) By the first law of thermodynamics A = Q - ΔU

or,  

Given    

So,    

(b)

Given  

or,  

or,  

or,    

Integrating both sides, we get

or,

or,    

or,  

or,  

Q32: Find the work performed by one mole of a Van der Waals gas during its isothermal expansion from the volume V₁ to V₂ at a temperature T. 

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Ans: The work done is

Q33: One mole of oxygen is expanded from a volume V₁ = 1.00 1 to V₂ = 5.0 l at a constant temperature T = 280 K. Calculate:
 (a) the increment of the internal energy of the gas: 
 (b) the amount of the absorbed heat.
 The gas is assumed to be a Van der Waals gas. 

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Ans: (a) The increment in the internal energy is

But from second law

On the other hand  

or,  

So,    

(b) From the first law  

Q34: For a Van der Waals gas find:
 (a) the equation of the adiabatic curve in the variables T, V;
(b) the difference of the molar heat capacities C_p, — C_v  as a function of T and V. 

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Ans: (a) From the first law for an adiabatic

dQ = dU + pd V = 0

From the previous problem

So,  

This equation can be integrated if we assume that Cv and b are constant then

or,  

(b)  We use  

Now,  

So along constant p,

Thus  

On differentiating,  

or,  

and  

Q35: Two thermally insulated vessels are interconnected by a tube equipped with a valve. One vessel of volume V₁ =  10 l contains v = 2.5 moles of carbon dioxide. The other vessel of volume V₂ = 100 l is evacuated. The valve having been opened, the gas adiabatically expanded. Assuming the gas to obey the Van der Waals equation, find its temperature change accompanying the expansion. 

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Ans: From the first law

as the vessels are themally insulated.

As this is free expansion,  

But  

So,  

or,  

Substitution gives ΔT = - 3 K

Q36: What amount of heat has to be transferred to v = 3.0 moles of carbon dioxide to keep its temperature constant while it expands into vacuum from the volume V₁ =  5.0 l to V₂ = 10 l ? The gas is assumed to be a Van der Waals gas. 

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Ans:   (as A = 0 in free expansion).

So at constant temperature.

= 0.33 kJ from the given data.