The Vander Waals equation for 0.5 mol of a g | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The general Vander Waals equation for $n$ moles of a gas is given by: $\left( P + \frac{an^2}{V^2} \right) \left( V - nb \right) = nRT$ Substituti

Vedclass · Accepted Answer

$\left( P + \frac{a}{4V^2} \right) \left( 2V - b \right) = RT$

Vedclass · Answer

(B) The general Vander Waals equation for $n$ moles of a gas is given by: $\left( P + \frac{an^2}{V^2} \right) \left( V - nb \right) = nRT$ Substituting $n = 0.5 = \frac{1}{2}$ mol into the equation: $\left( P + \frac{a(1/2)^2}{V^2} \right) \left( V - \frac{b}{2} \right) = \frac{1}{2} RT$ $\left( P + \frac{a}{4V^2} \right) \left( V - \frac{b}{2} \right) = \frac{RT}{2}$ Multiplying both sides by $2$: $\left( P + \frac{a}{4V^2} \right) \left( 2V - b \right) = RT$

The Vander Waals equation for $0.5 \ mol$ of a gas is:

Similar Questions

At very high pressures,the compressibility factor of one mole of a gas is given by

When does a real gas behave like an ideal gas?

Consider the following figure. Which of the following gases show negative as well as positive deviation from the ideal gas behaviour?

For a real gas,deviations from ideal gas behavior are maximum at:

If the compressibility factor $(Z)$ of a gas at $STP$ is greater than $1$,then what will be the value of its molar volume $(V_m)$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module