## Equation for Process Calculations for Ideal GasesEdit

For reversible, closed-system, work is given by

dW=-PdV

For ideal gases, the first law can be written by

dQ+dW=C_v dT

From two equations above, we get

dQ=C_v dT+PdV

These three equations can be applied to four types of processes: isothermal, isobaric, isochoric and adiabatic.

## Isothermal ProcessEdit

Isothermal process deals with closed-system that has constant temperature. So ΔT=0:

ΔU=ΔH=0

Q=RTln V_2/V_1 =-RTln P_2/P_1

W=-RTln V_2/V_1 =RTln P_2/P_1

Q=-W (constant T)

Therefore,

Q=-W=RT ln V_2/V_1 = -RT ln P_2/P_1 (constant T)

## Isobaric ProcessEdit

Isobaric process deals with closed-system that has constant pressure. So ΔP=0.

ΔU=∫▒〖C_v dT〗 and ΔH=∫▒〖C_p dT〗

Q=∫▒〖C_p dT〗 and W=-R(T_2-T_1)

Therefore,

Q=ΔH=∫▒〖C_p dT〗 (constant P)

## Isochoric ProcessEdit

Isochoric process deals with closed-system that has constant volume. So ΔV=0.

ΔU=∫▒〖C_v dT〗 and ΔH=∫▒〖C_p dT〗

Q=∫▒〖C_v dT〗 and W=-∫▒PdV=0

Therefore,

Q=ΔU=∫▒〖C_v dT〗 (constant V)

## Adiabatic ProcessEdit

Adiabatic process deals with closed-system that has no heat transfer between the system and the surroundings. So ΔQ=0.

dT/T= -R/C_v dV/V

T_2/T_1 =(V_1/V_2 )^(R⁄C_v )

T_2/T_1 =(P_2/P_1 )^(R⁄C_p ) and P_2/P_1 =(V_1/V_2 )^(C_p⁄C_v )

The following equations apply to ideal gases with constant heat capacities that undergo mechanically reversible adiabatic expansion or compression.

〖TV〗^(γ-1)=constant 〖TP〗^(((1-γ))⁄γ)=constant 〖PV〗^γ=constant

γ≡ C_p/C_v

For any adiabatic closed-system,

dW=dU= C_v dT

W= △U= C_v△T

γ ≡ C_p/C_v = (C_v+R)/C_v =1+ R/C_v or C_v= R/(γ-1)

W= C_v△T= (R△T)/(γ-1)

W= (〖RT〗_2-〖RT〗_1)/(γ-1)= (P_2 V_2-P_1 V_1)/(γ-1)

For mechanically reversible process,

W= (P_1 V_1)/(γ-1) [(P_2/P_1 )^(γ-1)-1]= (RT_1)/(γ-1) [(P_2/P_1 )^(((γ-1))⁄γ)-1]

## Diabatic ProcessEdit

Opposite of adiabatic process

There is heat transfer

## Polytropic ProcessEdit

Polytropic process deals with a model of some versatility. So δ=constant.

〖PV〗^δ=constant

〖TV〗^(δ-1)=constant 〖TP〗^(((1-δ))⁄δ)=constant

W= (RT_1)/(δ-1) [(P_2/P_1 )^(((δ-1))⁄δ)-1]

Q= ((δ-γ)RT_1)/((δ-1)(γ-1)) [(P_2/P_1 )^(((δ-1))⁄δ)-1]

## ReferenceEdit

Smith, J. M., and Ness H. C. Van. Introduction to Chemical Engineering Thermodynamics. New York: McGraw-Hill, 1987. Print.