Which among the following statements is/are i | vedclass

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Question

(D) Statement $(i)$ is incorrect because for real gases,$Z$ can be equal to $1$ at specific conditions (Boyle temperature).Statement $(ii)$ is correct

Vedclass · Accepted Answer

$(iii), (iv)$ only

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(D) Statement $(i)$ is incorrect because for real gases,$Z$ can be equal to $1$ at specific conditions (Boyle temperature).Statement $(ii)$ is correct because real gases behave ideally at low pressure and high temperature.Statement $(iii)$ is incorrect because real gases possess intermolecular forces of attraction.Statement $(iv)$ is incorrect because real gases obey the Van der Waals equation,$\left(P + \frac{an^2}{V^2}\right)(V - nb) = nRT$,not the ideal gas equation $PV = nRT$.Therefore,statements $(i), (iii),$ and $(iv)$ are incorrect. However,based on the provided options,$(iii)$ and $(iv)$ are clearly incorrect.

Similar Questions

Why do real gases deviate from ideal behavior in the $pV$ vs $p$ and $p$ vs $V$ graphs at specific temperatures?

Statement $-1$: The compressibility factor at the critical point is the same for different gases following van der Waal's equation.
Statement $-2$: The compressibility factor is independent of pressure at the critical temperature.

Explain the compressibility factor $(Z)$.

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

When is deviation more in the behaviour of a gas from the ideal gas equation $PV = nRT$?

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