A real gas most closely approaches the behavi | vedclass

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Question

(C) An ideal gas is a hypothetical gas whose pressure,volume,and temperature behaviour is described by the ideal gas equation. Real gases deviate from

Vedclass · Accepted Answer

$0.5 \, atm$ and $500 \, K$

Vedclass · Answer

(C) An ideal gas is a hypothetical gas whose pressure,volume,and temperature behaviour is described by the ideal gas equation. Real gases deviate from ideal behaviour due to the finite volume of gas particles and the existence of intermolecular forces. Real gases approach ideal behaviour under conditions of low pressure and high temperature. At low pressure,the volume of gas particles becomes negligible compared to the total volume. At high temperature,the kinetic energy of the particles is high enough to overcome the intermolecular forces of attraction. Comparing the given options,$0.5 \, atm$ (lowest pressure) and $500 \, K$ (highest temperature) provide the conditions where the real gas behaves most like an ideal gas.

$A$ real gas most closely approaches the behaviour of an ideal gas at

Similar Questions

$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$, what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?
$Z$ $\%$ Deviation

Van der Waal's equation $\left[ p + \frac{a}{V^2} \right] (V - b) = nRT$ is applicable for

Maximum deviation from ideal gas behavior is expected from which of the following gases?

Which gas shows real behavior?

Assertion : Compressibility factor $(Z)$ for non-ideal gases can be greater than $1$.
Reason : Non-ideal gases always exert higher pressure than expected.

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