Table of Contents
How enthalpy is function of pressure and temperature?
Just as internal energy, the enthalpy of a pure substance can be represented as a function of any two properties, or parameters, of state, for instance, of pressure p and temperature T: h = f (p, T). i.e. the enthalpy of an ideal gas does not depend on pressure.
What is enthalpy a function of in an ideal gas?
Since R is a constant and u = u(T), it follows that the enthalpy of an ideal gas is also a function of temperature only. Since u and h depend only on the temperature for an ideal gas, the constant volume and constant pressure specific heats cv and cp also depend on the temperature only.
Is enthalpy a function of pressure?
Enthalpy is the heat content of a system as a function of entropy and pressure. As the pressure increases ( ΔP>0 ), so does enthalpy, and vice versa. Enthalpy can still exist even at constant pressure; that describes the enthalpy of vaporization or fusion.
How are CP and CV related for an ideal gas?
The values indicated by Cp and Cv are the specific heats of an ideal gas. These indicate the quantity of heat that can increase the temperature of unit mass by 1°C. where, ΔQ is the amount of heat that is given to the system, ΔU is the change in internal energy and ΔW is the work done.
Why enthalpy is a function of temperature only for ideal gas?
For ideal gas, V equals to RT over P from the equation of state. Then, (dH over dP) at constant T becomes zero. Thus, enthalpy does not depend on pressure at constant T and it is a function of temperature only.
Why enthalpy of an ideal gas depends only on temperature?
Explanation: The enthalpy of an ideal gas depends only on the temperature because the internal energy of an ideal gas depends only on the temperature. Explanation: Change in enthalpy occurs when heat is given to a system at constant pressure.
Why the enthalpy of an ideal gas does depends only the temperature?
An ideal gas has no inter-molecular interactions. This means that the energy U of an ideal gas depends only on kinetic and not potential energy. As a result the energy U depends only on temperature T. The enthalpy H is defined as H=U+PV, but for an ideal gas PV=nRT so, for an ideal gas, H=U+nRT.
What is CV of an ideal gas?
The molar specific heat capacity of a gas at constant volume Cv is the amount of heat required to raise the temperature of 1 mol of the gas by 1◦C at the constant volume. Its value for monatomic ideal gas is 3R/2 and the value for diatomic ideal gas is 5R/2.
How do you calculate ideal gas CP?
The specific heat at constant volume is related to the internal energy U of the ideal gas by Cv=dUdT∣∣∣v=f2R, C v = d U d T | v = f 2 R , where f is degrees of freedom of the gas molecule.