How many L of chlorine gas, at STP, were required if 2.28 mol reacted?

Question

8H2S+8Cl2→S8+16HCl

How many L of chlorine gas, at STP, were required if 2.28 mol reacted?

Answer 1

Since the reaction takes place at STP (standard temperature and pressure), we know that 1 mole of an ideal gas equals 22.4 liters.

For this problem, we don't even need to use the stoichiometry of the balanced equation. It is simply using dimensional analysis to convert 2.28 moles of gas to liters using the conversion factor of 22.4 L/mole.

2.28 mol Cl₂ x 22.4 L/mole = 51.1 liters