Explain the effect of high pressure and low t | vedclass

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(B) Boyle's law states that for a fixed amount of an ideal gas at constant temperature,the pressure is inversely proportional to its volume $(P \propt

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Boyle's law shows significant deviations.

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(B) Boyle's law states that for a fixed amount of an ideal gas at constant temperature,the pressure is inversely proportional to its volume $(P \propto \frac{1}{V})$.High Pressure: At high pressure,the intermolecular forces of attraction become significant,and the volume of gas molecules is no longer negligible compared to the total volume. Consequently,real gases deviate from ideal behavior,and the $P$ vs $\frac{1}{V}$ plot is not a straight line.Low Temperature: At low temperatures,the kinetic energy of gas molecules decreases,making intermolecular forces more effective. This causes the gas to deviate from ideal behavior,and Boyle's law is not followed strictly.

Explain the effect of high pressure and low temperature on the validity of Boyle's law.

Similar Questions

For a real gas at $25^{\circ} C$ temperature and high pressure $(99 \ bar)$,the value of the compressibility factor is $2$. The value of the Van der Waals constant '$b$' is $\times 10^{-2} \ L \ mol^{-1}$. (Nearest integer) (Given $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

$A$ gas described by van der Waal's equation:

Define the compressibility factor $(Z)$ in terms of the molar volume of a gas.

The pressure $(p)$ and volume $(V)$ isotherm of a van der Waals' gas,at the temperature at which it undergoes gas to liquid transition,is correctly represented by

The pressure of real gases is less than that of ideal gas because of:

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