The molar heat capacity for the process shown in the figure is

Let us consider the figure given below :

We consider the process AB to be composed of two processes, AC(at constant pressure) and CB(at constant volume), such that AB = AC + CB. C is the molar heat capacity of AB, C_{p} is the molar heat capacity of AC(constant pressure) and Cv is the molar heat capacity of CB(constant volume).

From the first law of thermodynamics, we know that Q = U + W … (i),

Where Q = heat supplied, U = change in internal energy, W = work done on the system.

Since the change in internal energy is independent of the path, it will have the same value for paths AB and ACB.

Hence, U_{AB} = U_{ACB} … (ii), where U_{AB} = change in internal energy for path AB, U_{ACB} = change in internal energy for path ACB.

Now, the work done by a process is given by the area under the PV diagram. We can clearly see that the area under process AB is greater than the sum of areas under processes AC and CB.

Hence, W_{AB} > W_{ACB} … (iii), where W_{AB} = work done for process following path AB, W_{ACB} = work done for process following path ACB.

Adding (ii) and (iii), we get :

U_{AB} + W_{AB} > U_{ACB} + W_{ACB} … (iv)

But, from the first law of thermodynamics, Q = U + W, where Q = heat supplied, U = change in internal energy, W = work done on the system.

Hence, we get, Q_{AB} > Q_{ACB} … (v),

We know, Q_{AB} = nCdT, Q_{AC} = nC_{p}dT, Q_{CB} = nC_{v}dT,

where Q_{AB} = heat supplied in process AB

Q_{AC} = heat supplied in process AC

Q_{CB} = heat supplied in process CB

n = number of moles

C = molar heat capacity

C_{p} = molar heat capacity at constant pressure

C_{v} = molar heat capacity at constant volume

dT = change in temperature.

Also, Q_{ACB} = Q_{AC} + Q_{CB} … (vi), where

Q_{ACB} = heat supplied in process ACB

Q_{AC} = heat supplied in process AC

Q_{CB} = heat supplied in process CB

Hence, from (v), we get,

nCdT > nC_{p}dT + nC_{v}dT

Dividing by ndT on both sides :

C > C_{p} + C_{v} => C > C_{v} (option c)

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