The characteristic equation of gases PV=nRT holds good for:(A) Monoatomic gases(B) Diatomic gas(C) Real gases(D) Ideal gases

The ideal gas law, PV = nRT, can be applied to all gases, but its accuracy may vary depending on the type of gas and the conditions under which it is used. Let's break down the options:

(A) Monoatomic gases: The ideal gas law can be applied to monoatomic gases under certain conditions, especially at low pressures and high temperatures. However, deviations from ideal behavior may become more significant at high pressures and low temperatures.

(B) Diatomic gases: Similar to monoatomic gases, diatomic gases can also be described by the ideal gas law under certain conditions. Again, deviations from ideal behavior become more pronounced at extreme conditions.

(C) Real gases: Real gases do not strictly obey the ideal gas law at all conditions. Real gases exhibit deviations from ideal behavior, particularly at high pressures and low temperatures. Under these conditions, intermolecular forces and molecular volume effects become more significant.

(D) Ideal gases: The ideal gas law, PV = nRT, is an idealized equation that assumes no intermolecular forces and negligible molecular volume. Ideal gases do not exist in reality but are used as a convenient approximation for many gases under typical laboratory conditions (moderate pressures and temperatures).

So, the correct answer is:

(D) Ideal gases

However, it's important to note that for real gases and non-ideal conditions, more complex equations of state like the van der Waals equation or the Virial equation may be more appropriate to describe their behavior accurately.