Small gas tanks are often used to supply gases for chemistry reactions. A gas gauge will give some information about how much is in the tank, but quantitative estimates are needed so that the reaction will be able to proceed to completion. Knowing how to calculate the necessary parameters for gases is very helpful to avoid running out earlier than desired.

## Conversions Between Moles and Gas Volume

Molar volume at STP can be used to convert from moles to gas volume and from gas volume to moles. The equality of \(1 \: \text{mol} = 22.4 \: \text{L}\) is the basis for the conversion factor.

Example \(\PageIndex{1}\)

Many metals react with acids to produce hydrogen gas. A certain reaction produces \(86.5 \: \text{L}\) of hydrogen gas at STP. How many moles of hydrogen were produced?

**Solution**

*Step 1: List the known quantities and plan the problem.*

__Known__

- \(86.5 \: \text{L} \: \ce{H_2}\)
- \(1 \: \text{mol} = 22.4 \: \text{L}\)

__Unknown__

Apply a conversion factor to convert from liters to moles.

*Step 2: Calculate.*

\[86.5 \: \text{L} \: \ce{H_2} \times \frac{1 \: \text{mol} \: \ce{H_2}}{22.4 \: \text{L} \: \ce{H_2}} = 3.86 \: \text{mol} \: \ce{H_2}\nonumber \]

*Step 3: Think about your result.*

The volume of gas produced is nearly four times larger than the molar volume. The fact that the gas is hydrogen plays no role in the calculation.

Example \(\PageIndex{2}\)

What volume does \(4.96 \: \text{mol}\) of \(\ce{O_2}\) occupy at STP?

**Solution**

*Step 1: List the known quantities and plan the problem*.

__Known__

- \(4.96 \: \text{mol} \: \ce{O_2}\)
- \(1 \: \text{mol} = 22.4 \: \text{L}\)

__Unknown__

*Step 2: Calculate.*

\[4.96 \: \text{mol} \times 22.4 \: \text{L/mol} = 111.1 \: \text{L}\nonumber \]

*Step 3: Think about your result.*

The volume seems correct given the number of moles.

Example \(\PageIndex{3}\)

If we know the volume of a gas sample at STP, we can determine how much mass is present. Assume we have \(867 \: \text{L}\) of \(\ce{N_2}\) at STP. What is the mass of the nitrogen gas?

**Solution**

*Step 1: List the known quantities and plan the problem.*

__Known__

- \(867 \: \text{L} \: \ce{N_2}\)
- \(1 \: \text{mol} = 22.4 \: \text{L}\)
- Molar mass \(\ce{N_2} = 28.02 \: \text{g/mol}\)

__Unknown__

*Step 2: Calculate.*

We start by determining the number of moles of gas present. We know that 22.4 liters of a gas at STP equals one mole, so:

\[867 \: \text{L} \times \frac{1 \: \text{mol}}{22.4 \: \text{L}} = 38.7 \: \text{mol}\nonumber \]

We also know the molecular weight of \(\ce{N_2}\) \(\left( 28.0 \: \text{g/mol} \right)\), so we can then calculate the weight of nitrogen gas in 867 liters:

\[38.7 \: \text{mol} \times \frac{28 \: \text{g}}{1 \: \text{mol}} = 1083.6 \: \text{g} \: \ce{N_2}\nonumber \]

*Step 3: Think about your result.*

In a multi-step problem, be sure that the units check out.