# Question 4c1cf

Aug 14, 2016

The pressure of the gas is 26 atm.

#### Explanation:

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

color(blue)(|bar(ul(PV = nRT)|),

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

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

$n = \text{4.95 mol}$
$R = \text{0.082 06 L·atm·K"^"-1""mol^"-1}$
$T = \text{(75 + 273.15) K = 348.15 K}$
$V = \text{5.4 L}$

P = (nRT)/V = (4.95 color(red)(cancel(color(black)("mol"))) × "0.082 06" color(red)(cancel(color(black)("L")))"·atm·"color(red)(cancel(color(black)("K"^"-1""mol"^"-1"))) × 348.15 color(red)(cancel(color(black)("K"))))/(5.4 color(red)(cancel(color(black)("L")))) = "26 atm"#