# The concentration of #CO_2# in a can of soda is approximately 0.045 M. If all of the #CO_2# in a 12 ounce soda evolves from solution, how many liters would the #CO_2# gas take up at STP?

##### 1 Answer

#### Answer:

#### Explanation:

The idea here is that you need to figure out how many **moles** of carbon dioxide, *volume* and *molarity* of the solution.

As you know, a **molarity** of **every liter** of solution, which in your case is soda, will contain **moles** of carbon dioxide.

This means that your

#12 color(red)(cancel(color(black)("oz"))) * (29.57 color(red)(cancel(color(black)("mL"))))/(1color(red)(cancel(color(black)("oz")))) * "1 L"/(10^3color(red)(cancel(color(black)("mL")))) = "0.35484 L"#

sample of soda will contain

#0.35484 color(red)(cancel(color(black)("L soda"))) * "0.045 moles CO"_2/(1color(red)(cancel(color(black)("L soda")))) = "0.01597 moles CO"_2#

Now, you are told that **all of the moles** of carbon dioxide evolve from the solution.

As you know, **STP conditions**, which are defined as a pressure of **one mole** of any ideal gas occupies exactly **molar volume of a gas at STP**.

This means that your sample of carbon dioxide will occupy

#0.01597 color(red)(cancel(color(black)("moles CO"_2))) * "22.7 L"/(1color(red)(cancel(color(black)("mole CO"_2)))) = color(green)(|bar(ul(color(white)(a/a)color(black)("0.36 L")color(white)(a/a)|)))#