# Question 59112

Jun 24, 2017

The volume at STP is 471 L.

#### Explanation:

Step 1. Calculate the moles of ${\text{CO}}_{2}$

$\text{Moles of CO"_2 = 1.25 × 10^25 color(red)(cancel(color(black)("molecules"))) × "1 mol"/(6.022 ×10^23 color(red)(cancel(color(black)("molecules")))) = "20.76 mol}$

Step 2. Calculate the volume of ${\text{CO}}_{2}$

I assume that the gas is at STP (1 bar and 0 °C).

We can use the Ideal Gas Law to calculate the volume.

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

We can rearrange this to

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

V = (20.76 color(red)(cancel(color(black)("mol"))) × "0.083 14" color(red)(cancel(color(black)("bar")))·"L"·color(red)(cancel(color(black)("K"^"-1""mol"^"-1"))) × 273.15 color(red)(cancel(color(black)("K"))))/(1 color(red)(cancel(color(black)("bar")))) = "471 L"#