Chapter 5, Problem 5.10P

Interpretation Introduction

(a)

Interpretation:

The pressure guage on a $20.0{\text{ m}}^3$ tank of nitrogen at ${25}^{\text{o}}\text{C}$ reads $10.0\text{ bar}$. The mass of nitrogen in the tank by direct solution of the ideal-gas equation of state should be calculated.

Concept introduction:

The ideal gas law can be used to find out the amount of nitrogen and then multiply it by the molar mass of nitrogen to find the mass of nitrogen in the tank.

$PV =nRT$

Where,

$P$ - Pressure

$V$ - Volume

$T$ - Temperature

$n$ - Number of moles of gas

$R$ - Ideal gas constant

Interpretation Introduction

(b)

Interpretation:

The pressure guage on a $20.0{\text{ m}}^3$ tank of nitrogen at ${25}^{\text{o}}\text{C}$ reads $10.0\text{ bar}$. The mass of nitrogen in the tank by conversion from standard conditions should be calculated.

Concept introduction:

When we consider the conversion from the standard condition, then we have to assume that nitrogen is not a ideal behaving gas and then we have to use the van der waal’s equation for slove this problem.

$\left[p+a{\left(\frac{n}{v}\right)}^2\right]\left[v–nb\right]=nRT$

Where,

$p$ - Pressure

$v$ - Volume

$T$ - Temperature

$n$ - Number of moles of gas

$R$ - Ideal gas constant

$\left(a,b\text{ are specific constants for each gas}\right)$