Which among the following statements is/are incorrect regarding real gases?
(i) Their compressibility factor is never equal to unity $(Z \neq 1)$ .
(ii) The deviations from ideal behavior are less at low pressures and high temperatures.
(iii) Intermolecular forces among gas molecules are equal to zero.
(iv) The obey Van der Waals equation, $PV = nRT$ .

Question

Which among the following statements is/are incorrect regarding real gases?
(i) Their compressibility factor is never equal to unity

(Z \neq 1)

.
(ii) The deviations from ideal behavior are less at low pressures and high temperatures.
(iii) Intermolecular forces among gas molecules are equal to zero.
(iv) The obey Van der Waals equation,

PV = nRT

.

Aicharya · Accepted Answer

At high pressure, the gas molecules come close to each other and the empty space between the molecules is reduced to some extent. Therefore the gas becomes less compressible at these higher pressures

For the real gas equation is

$(P + \frac{a}{{nV}^{2}}) (V - nb) = RT$

Thus, Intermolecular force among the gas molecule which is not equal to zero

Whereas the equation of vendrawall's equation is

$(P + \frac{a^{2}}{n^{2} V^{2}}) (V - nb) = RT$

So from above theory the incorrect option is $(iii) & (iv)$

Which among the following statements is/are incorrect regarding real gases? (i) Their compressibility factor…

Solution