Which of the following statements is false ba | vedclass

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(D) The compressibility factor $Z$ is defined as $Z = \frac{PV}{nRT}$.For a van der Waals gas,the equation is $(P + \frac{an^2}{V^2})(V - nb) = nRT$.A

Vedclass · Accepted Answer

The dashed curve represents an ideal gas where $a = 0$ and $b = 0$.

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(D) The compressibility factor $Z$ is defined as $Z = \frac{PV}{nRT}$.For a van der Waals gas,the equation is $(P + \frac{an^2}{V^2})(V - nb) = nRT$.At low pressure,$Z \approx 1 - \frac{a}{RTV}P$,which explains the initial decrease in $Z$ for real gases (where $a > 0$).At high pressure,$Z \approx 1 + \frac{Pb}{RT}$,which explains the increase in $Z$ for real gases (where $b > 0$).Gas $A$ shows $Z > 1$ for all $P$,implying $a = 0$ and $b > 0$.Gas $B$ shows $Z  0$ and $b = 0$.The dashed curve represents a typical real gas where both $a$ and $b$ are non-zero.Therefore,the statement that the dashed curve represents an ideal gas is false.

Which of the following statements is false based on the provided graph of compressibility factor $Z$ versus pressure $P$?

Similar Questions

Consider the equation $Z = \frac{PV}{RT}.$ Which of the following statements is correct?

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