Real gases do not follow the ideal gas equation perfectly under all conditions . They show deviation from the ideal behavior when

Options

A. pressure is high and temperature is low
B. pressure is low and temperature is high
C. both pressure and temperature are high
D. both pressure and temperature are low

Answer

A

Explanation

Real gases do not follow Boyle's law, Charles'law , and Avogadro's law perfectly under all conditions on account of intermolecular interactions which become significant when their molecules are quite close (due to high pressure) and are moving very slowly (due to low temperature). The deviation from ideal behavior becomes apparent when the pressure vs. volume plot is drawn.

It is apparent that at very high pressure, the measured volume for real gases is more than the calculated volume (from Boyle's law) for ideal gases. At low pressures, measured and calculated volumes approach each other.
The nonideal behavior(deviation from the predictions of the ideal gas laws) is most significant at high pressures and//or low temperatures, that is, near the conditions under which the gas liquefies.