IDEAL GAS EQUATION

If E is the energy density in an ideal gas, then the pressure of the ideal gas is

If P, V, M, T and R are symbols of pressure, volume, molecular weight, temperature and Gas contstant, what is the equation of density of ideal gas

Assertion (A): The Joules -Thomon coefficient for an ideal gas is zero. Reason (R ) : There are no intermlecular attactive forces in an ideal gas.

Assertion (A): The Joules -Thomon coefficient for an ideal gas is zero. Reason (R ) : There are no intermlecular attactive forces in an ideal gas.

For an ideal gas the equation of a process for which the heat capacity of the gas varies with temperatue as C=(alpha//T(alpha) is a constant) is given by

Assertion : Compressibility factor for ideal gas is one. Reason : For an ideal gas PV = nRT equation is obeyed.

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT AT relatively high pressures, the van der Waals' equation of state reduces to

The gases obey the different gas laws only theoretically. Practically all of them show some deviation from these laws. These are called real gases. The deviation are maximum under high pressure and at low temperature. These are comparatively small when the conditions are reversed. It has been found that the easily liquefiable gases show more deviations from the ideal gas behaviour as compared to the gases which are liquified with difficulty. The van der Waals equation reduces itself to ideal gas equation at

According to the real gas equation, Z is equal to 1 for an ideal gas and Z is variable for a real gas. Suppose, in order to easy our calculation, we fixed Z=1 for real gas and for ideal gas Z will become variable, Z vs P for an ideal gas will be similar to:

A gas behaves as an ideal gas at