# A chemical reaction occurring in a cylinder equipped with a moveable piston produces 0.58 mol of a gaseous product. If the cylinder contained 0.11 mol of gas before the reaction and had an initial volume of 2.1L, what was its volume after the reaction?

##### 1 Answer

The new volume of the cylinder will be equal to **13 L**.

When no mention of pressure or temperature is made, you can assume that they are kept constant. This means that you can use Avogadro's Law to determine what the new volume of the cylinder will be.

According to Avogadro's Law, the volume of a gas is *directly proportional* to the number of moles of gas present, when temperature and pressure are kept constant.

In other words, the *bigger* the number of moles of gas present, the *bigger* the volume. Think about blowing up a balloon. The more you put into it, the bigger its volume gets.

Mathematically, this relationship is expressed like this

You know that your reaction produces **0.58 moles** of gas, and that **0.11 moles** of gas were *already* in the cylinder. This means that the *total number of moles* present in the cylinder after the reaction is completed will be

Use the above equation to solve for

Rounded to two sig figs, the answer will be