The deviation from the ideal gas equation PV | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) Real gases deviate from ideal behavior because of intermolecular forces and the finite volume of gas molecules. These deviations become significan

Vedclass · Accepted Answer

Low temperature and high pressure

Vedclass · Answer

(B) Real gases deviate from ideal behavior because of intermolecular forces and the finite volume of gas molecules. These deviations become significant when the gas molecules are close together and moving slowly. This occurs at $Low \ temperature$ (where kinetic energy is low) and $High \ pressure$ (where molecules are compressed into a smaller volume). Therefore,the deviation from the ideal gas equation $PV = nRT$ is maximum at $Low \ temperature$ and $High \ pressure$.

The deviation from the ideal gas equation $PV = nRT$ is maximum under which of the following conditions?

Similar Questions

Identify the correct variation of pressure $(p)$ and volume $(V)$ of a real gas $(A)$ and an ideal gas $(B)$ at constant temperature. ($y = p$; $x = V$)

The van der Waals equation of state for a real gas is given. For $n$ moles of a real gas,the equation can be expressed as:

$A$ gas at $350 \; K$ and $15 \; bar$ has a molar volume $20$ percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor $(Z)$ is

The pressure of a van der Waals gas is less than the pressure of an ideal gas because of

Four gases $P, Q, R$ and $S$ have almost same values of $b$ but their $a$ values ($a, b$ are van der Waals' constants) are in the order $Q < R < S < P$. At a particular temperature among the four gases,the most liquefiable one is

Vedclass Test Series

Exam Paper Generator

Online Exam Module