Question

Which of the following statements is NOT correct? The PV/nRT ratio for real gases can be greater than 1 because of the attractive forces between molecules. Real gases deviate from ideal gases because of the finite size of the molecules and the attractive and repulsive interactions between molecules. Gases often deviate from ideal behavior at sufficiently high pressures and low temperatures. A decrease in temperature causes a decrease in gas pressure because the frequency of molecules colliding with the wall decreases. An increase in pressure is observed as temperature of a gas increases because the average force of molecules colliding with the wall increases.

Answer 1

Answer:

None of the statements is incorrect

Explanation:

Real gases behave ideally at high pressure and low temperature.

This is due to the increase in intermolecular force of attraction between gaseous molecules at high pressure.

$\dfrac{PV}{RT}$ ratio is equal to one for ideal gases where it is greater than or less than 1 for real gases.

When the temperature increases, the number gaseous molecules colliding the walls of container will also increase thus increasing the pressure of gas.