# Question ad885

May 9, 2017

The pressure of the gas is 192 bar.

#### Explanation:

This looks like the time to apply the Ideal Gas Law:

$\textcolor{b l u e}{\overline{\underline{| \textcolor{w h i t e}{\frac{a}{a}} p V = n R T \textcolor{w h i t e}{\frac{a}{a}} |}}} \text{ }$

where

• $p$ is the pressure
• $V$ is the volume
• $n$ is the number of moles
• $R$ is the gas constant
• $T$ is the temperature

We can rearrange the Ideal Gas Law to get

$P = \frac{n R T}{V}$

In this problem,

$n = \text{4.35 mol}$
$R = \text{0.0831 4 bar·L·K"^"-1""mol"^"-1}$
$T = \text{(75 + 273.15) K" = "348.15 K}$
$V = \text{0.655 L}$

P = (4.35 color(red)(cancel(color(black)("mol"))) × "0.083 14 bar"·color(red)(cancel(color(black)("L·K"^"-1""mol"^"-1"))) × 348.15 color(red)(cancel(color(black)("K"))))/(0.655 color(red)(cancel(color(black)("L")))) = "192 bar"#