van der Waal's equation reduces itself to the ideal gas equation at

Options

A. high pressure and low temperature
B. low pressure and low temperature
C. low pressure and high temperature
D. high pressure alone

Answer

C

Explanation

At low pressure , the distance between the molecules is large. At high temperatures , these molecules are moving wit great speeds. Under these conditions , intermolecular interactions are minimum. Thus , a real gas behaves like an ideal gas and the van der Waals equation reduces itself to the ideal gas equation.