To answer this question, you must use the **ideal gas equation**:

P V = n R T

"P" stands for **pressure**, "V" stands for **volume**, "n" stands for **number of moles**, "R" stands for **gas constant**, and "T" stands for **temperature**.

The problem mentions that this scenario occurs at STP, which stands for **standard temperature and pressure**. This automatically gives us two important pieces of information: (1) the temperature in the scenario is 273 K & (2) the pressure in the scenario is 1 atm.

It's also given to us that there are 4.4 g of CO2 present in the scenario, which can help us to calculate the number of moles! By looking at the periodic table, we can see that 1 mole of carbon has a mass of 12.011 g & 1 mole of oxygen has a mass of 15.999 g. Since 1 mole of CO2 is composed of 1 mole of carbon and 2 moles of oxygen, we can find that 1 mole of CO2 has a mass of 44.009 g.

`(12.011 g) + 2 xx (15.999 g) = 44.009 g`

We then use the **molar mass** of CO2 to find the number of moles:

`(4.4 g)/1 xx (1 mol)/(44.009 g) = 0.10 mol`

The gas constant -- "R" -- is a constant, and we choose which ones to use based on the other **units** in our scenario. Since this scenario deals with atm, K, and mol, we will use the following for "R":

`R = 0.08206 (L atm)/(mol K)`

Now we can put everything we know into the ideal gas equation & solve for volume:

`(1 atm) xx V = (0.10 mol) xx (0.08206 (L atm)/(mol K)) xx (273 K)`

`V = 2.2 L`