Cp and Cv are specific heats at constant pressure and constant volume, respectively. It is observed that Cp − Cv =a for hydrogen gas Cp − Cv =b for nitrogen gas. The correct relation between a and b is :
Cp and Cv are specific heats at constant pressure and constant volume, respectively. It is observed that Cp − Cv =a for hydrogen gas Cp − Cv =b for nitrogen gas. The correct relation between a and b is :
In a system, Cp is the amount of heat energy released or absorbed by a unit mass of the substance with the change in temperature at a constant pressure.During a small change in the temperature of a substance, Cv is the amount of heat energy absorbed/released per unit mass of a substance where volume does not change.
The following relationship can be given considering the ideal gas behaviour of a gas. Cp – Cv = R
where R has been called universal gas constant.
For any gas, Cp−Cv = R, which is the gas constant.
Hence be it any gas, hydrogen or nitrogen, its value is same.
Here, for ideal gas, Cp – Cv = R/M, where M is the mass of one mole of gas.
Mass of one mole of hydrogen M=2 g and that of nitrogen M=28 g
∴ a=Cp−Cv=R/2 (for hydrogen)
And b=Cp−Cv=R/28 (for nitrogen)
⟹ a=14b
In a system, Cp is the amount of heat energy released or absorbed by a unit mass of the substance with the change in temperature at a constant pressure.During a small change in the temperature of a substance, Cv is the amount of heat energy absorbed/released per unit mass of a substance where volume does not change.
The following relationship can be given considering the ideal gas behaviour of a gas. Cp – Cv = R
where R has been called universal gas constant.
For any gas, Cp−Cv = R, which is the gas constant.
Hence be it any gas, hydrogen or nitrogen, its value is same.
Here, for ideal gas, Cp – Cv = R/M, where M is the mass of one mole of gas.
Mass of one mole of hydrogen M=2 g and that of nitrogen M=28 g
∴ a=Cp−Cv=R/2 (for hydrogen)
And b=Cp−Cv=R/28 (for nitrogen)
⟹ a=14b
