Specific heat of a gas is same in both isochoric and isobaric process

The Palchoudhury gas theory and Palchoudhury gas equation have a profound potency applicable to all phenomena of gases. Inner and covered outer surface area of molecules are the outstanding inventions related to gas behaviour. The exertion of infrared wave force on the covered outer surface area of tiny particles and the corresponding effect on the inner surface of a gas container is the real cause of the gas behaviour. We can independently explain all kind of behaviour of gases with the help of the conception the inner force and internal force. We can clarify about the isothermal and adiabatic behaviour of gases, show the relation between heat and force. It is most significant finding, the specific heat of an identical gas in the isochoric and the isobaric process is not different but same as the inner force in both methods is same.


INTRODUCTION
Heat, i.e. infrared wave call it as the heat wave.Heat wave holds some force during play up and down in the universe like an ocean wave.Heat wave exerts some force on the outer surface of tiny particles like atoms, molecules, etc.And in turn, the corresponding force consecutively and cumulatively uses an effect on the inner surface of a closed gas container.Every heat wave holds some energy that transfers to the gases and gases become hot.Again, some external force applies to gas that forces transfers into the heat of gases.It is comprehensive text, and the gases have no specific shape and size.According to Palchoudhury gas theory Palchoudhury (2016), the gas behaviour depends only on four variable (Pressure, temperature, inner surface area and outer surface area).Four variables compatible with Van der Waals constant and fit in all process-like the isochoric, isobaric, isothermal and adiabatic process of gases.

ANALYSIS OF ISOCHORIC AND ISOBARIC PROCESS
On in-depth analysis of the isochoric and isobaric processes of gases shown in the Table 1 and Table 2, reveals the following information, a) The inner force of the identical gases is the same in both isochoric and isobaric process on increment 1 oK temperature.b) The inner force of gases in the isochoric and isobaric process is different for different gases.It is remarkable, the inner force in the isochoric and isobaric process is different for the different size (inner surface area) of same gas as shown for carbon dioxide in Table1 and 2. c) For increment 1 oK temperature of gases, the internal force of the isochoric process is comparatively higher than isobaric process shown in Table 1 and Table 2.The excess internal force as seen in the isochoric process, the same spends for expanding the inner surface area in the isobaric process and the force remains as a static force (see the Table 2).d) Per unit internal force which depends on the covered outer surface of a substance and the inner surface area is a field intensity of gases.e) The equal heat wave force requires during the increment of 1 oK temperature of gases as found inner force is the same in both for the isochoric and isobaric processes shown in Table 1 and Table 2.

REGARDING HEAT CAPACITY OF GASES
There is an excellent role of size (inner surface area) of a gas in the effect of inner and internal force on increasing 1 oK temperature of gases.In Table 1 and Table 2 reveals, the inner force effects heavily on the smallest inner surface area than the larger inner surface area as seen for one-mole carbon dioxide gas.Much more heat wave force requires for the smallest inner surface area than the larger inner surface area to rise 1 oK temperature of gases.According to the Palchoudhury gas equation  =  where  here is pressure,  Inner surface area,  is constant of proportionality,  is number of moles,  covered outer surface area of molecules and  is temperature, Palchoudhury (2016)  = , that  is the inner force (Palchoudhury, 2017a(Palchoudhury, , 2017b)), corresponding to heat depends on the product of pressure and inner surface area.Again,  ∝ T, the inner force corresponding to heat depends on the outcome of the covered outer surface area of tiny particles and temperature.There is a significant role of the substance per unit inner surface area in the effect of gas behaviour as the internal force depends on the covered outer surface area of the substance.The ratio of internal force which depends on the elements, and the inner surface area have a significant role in the behaviour of gases.The specific heat of gases is a comparative matter.We may use any gas as a mediator.General text in the standard textbook, 1 cal = 4.18 J and Cvm (Isochoric)= H = 4.82 cal/mole O K for Carbon monoxide, and we may treat it as corresponding Csm (Isochoric)= H = 4.82 cal/mole-K (Heat capacity under constant inner surface area of one mole carbon monoxide).Therefore, H = 4.82 /cal for one mole Carbon monoxide.Now, so that  is inner force,  is heat and  is nominated as the constant of proportionality.On conceptual based argument, we may accept carbon monoxide (CO) as a mediator.Now, for one mole Carbon monoxide at temperature, 274 ok and with inner surface area of 1.65 dm 2 (square decimeter), covered outer surface area of 0.009 dm 2 , and pressure 10.45  (Mega Pascal), when for increasing 1  (from 273 oK to 274 oK ) in temperature, increase of the inner force  = 630.77N mole K (column-13/100) in Table 1 and when Csm = H = 4.82 cal/mole-K then, =130.73N/cal (about).In this paper we have used the following phrases in all Tables, as below; 1-The common gases are as, Co2 , He, Ne, H, Ar, O, N, Co, CH4 and NH3 .

2-
The volume for the gases, He, Ne, H, Ar, O, N, Co, CH4 and NH3 is 0.2 and for Co2 , is 0.05, 0.2 and 22.4 in SI unit.
3-We have selected one mole ( = 1) for all gases.

6-
The temperature  is 273 oK , and the inner force of the identical gases is the same in both isochoric and isobaric process on increment 1 oK .

7-
Here   and   are the forces on whole inner surface area before and after increment 1 oK , respectively in SI unit (/ 2 ).

8-
The difference between the forces, defined by ∆ =   −   and is in the SI unit (/ 2 ).

9-
The   is defined as the internal force on the outer surface  covered outer surface area of molecules of gases by heat wave force and following the below, 10-Here   is the specific heat capacity of gases in Kcal and then the Heat of gases is the heat of gases after increment of 1 k temperature of gases bears total heat in kcal.This value will be producing by, (5) 11-Moreover the heat on outer surface is the heat of outer the surface after increment 1 K temperature, outer surface of molecules bear total heat in Kcal and is and mentioned as H  in the table.Data (column 1 to 4) collected from (Palchoudhury, 2017a).  =  −   , H  is the convert into heat of   .

CONCLUSION
The result of this work show that there is no difference in specific heat of a gas in the isochoric and isobaric process.It is necessary to mention that the inner force in both processes is same due to effect of heat wave force.

Table 1 .
The relation between force and heat in isochoric process for individual gases and heat capacity of gases.

Table 2 .
The relation between force and heat in isobaric process for individual gases and heat capacity of gases.
and   are the inner surface area before and after temperature increment with 1 oK .()=   of Table1minus   of Table2.

Table 3 .
Behaviour of gases under compression and expansion in isothermal process.

Table 4 .
is the difference between   and   and H  is the convert into heat of   Behaviour of gases under compression and expansion in adiabatic process   = 273° ,   = 261.13°, [here subscripts (be) and (af) indicates the before and after the expansion of the gas respectively]