Because Cp has two functions:-
1-To change the internal energy dU.
2-To do work dW in expanding the gas.
Where as Cv has only one function of changing the internal energy of the gas..by awais
Cp=cv
cp-cv =R proved that//
Because Cp has two functions:- 1-To change the internal energy dU. 2-To do work dW in expanding the gas. Where as Cv has only one function of changing the internal energy of the gas....by Hamoud Seif
1.005
Cv is a for a constant volume, and there is therefore no work done in the expansion whereas as Cp accounts for the work done by the gas during its expansion, as well as the change in its internal energy. Thusly Cp is generally bigger than Cv. Intuitively this would be very simple to work out yourself. We used to have to work this out ourselves back in my day, not just resort to cheap answers on the interweb.
No, this relation is ONLY for ideal gases. The difference between Cp and Cv can be written more generally as T*(dP/dT)v*(dV/dT)p, where the lower case v and p represent the derivatives taken at constant volume and pressure, respectively. If you take these two derivatives using the ideal gas law (PV=nRT), then the result simplifies to Cp-Cv=R. However, solids and liquids do not follow the ideal gas law, and the difference between Cp and Cv is much smaller... negligible in many cases. For solids, Cp-Cv can be calculated using the isobaric expansivity, isothermal compressibility, and density of the material.
= 1 - qout/qin = 1 - cv(T4-T1)/(cv(Tx-T2)+cp(T3-Tx))
To find the atomicity of an ideal gas you can use γ = Cp/Cv.
Cp-Cv is the relation of Mayer's formula. It can also be defined in words as the difference between two specific heat capacities.
(rho/potential_density) = (p/reference pressure)^(1/gamma) where gamma is the ratio of specific heats Cp/Cv = 1.40.
When goods are normal, CV > EV.
Gasses have two specific heat capacities because the boundary conditions can affect the number by up to 60%. Therefore, a number is given to each boundary condition: isobaric (constant pressure) or isochoric (constant volume). In an ideal gas, they differ by the quantity R (the gas constant - the same one you use in the ideal gas law): Cp = Cv + R where Cp is the isobaric molar heat capacity (specific heat) and Cv is the isochoric molar heat capacity.