Chapter 5, Problem 5.35P

Interpretation Introduction

Interpretation:

The pressure of $1.47\times {10}^{-3}\text{mol}$ of argon contained in $75.0\text{mL}$ container at $26°\text{C}$ is to be calculated.

Concept introduction:

Ideal gas law equation is as follows:

$PV=nRT$ (1)

Here,

$P$ is the pressure of the gas.

$V$ is the volume occupied by gas.

$n$ is the no. of moles of gas.

$T$ is the temperature in Kelvin.

$R$ is the universal gas constant.

Conversion factor to convert $\text{mL}$ to $\text{L}$ is as follows:

$1\text{ml}={10}^{-3}\text{L}$

Conversion factor to convert $\text{atm}$ to $\text{torr}$ is as follows:

$1\text{atm}=760\text{torr}$

The conversion factor to convert $°\text{C}$ to Kelvin is as follows:

$T\left(\text{Kelvin}\right)=T\left(\text{°C}\right)+273.15$ (2)