# Calculate the volume of hydrogen required for complete hydrogenation of 0.25 #dm^3# of ethyne at STP?

##### 1 Answer

#### Answer:

You'd need

#### Explanation:

Like with any stoichiometry problem, the key tool you have at your disposal is the mole ratio.

However, an interesting thing takes place when you're dealing with gases that are *under the same conditions* for pressure and temperature. In such cases, the mole ratio becomes the **volume ratio**.

The idea is that, since you're dealing with two ideal gases, you can use the ideal gas law equation to write

The pressure and the temperature are the same for both gases, since the reaction presumably takes place at **STP**.

If you divided these two equations, you'll get

This is equivalent to

The mole ratio is equivalent to the volume ratio.

All you need now is the balanced chemical equation for the reaction, which looks like this

Notice that you have a **twice as many** moles of hydrogen gas than of ethyne.

This translates into volumes as well. In other words, the volume of hydrogen gas must be **twice as big** as the volume of ethyne.