An investigation about the molar volume of hydrogen gas at stp
Created by: Krish Chowdhary, Sherry Kuang, David Liu, Allen Chan

An investigation about the molar volume of hydrogen gas at stp
Created by: Krish Chowdhary, Sherry Kuang, David Liu, Allen Chan

For: SCH3U0, Mr. Martin
Completed:
For: SCH3U0, Mr. Martin
Completed:

Introduction
In this experiment, the objective is to prove the the molar volume of hydrogen at STP using the concept of gas stoichiometry learned in class, combined with hands on experimentation. The experiment was started with a small sample of magnesium and ten to fifteen mL of hydrochloric acid. Hydrogen gas (H2) is expected to be produced through a single displacement reaction, shown in the chemical formula below, using magnesium (the limiting reagent) and aqueous hydrochloric acid:
Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)

A graduated cylinder containing water, hydrochloric acid, and a piece of magnesium ribbon held into place by copper wire is to be inverted and placed into a beaker of water. As the acid is denser than water, it will remain at the bottom of the tube when upside down. The reaction is expected to take place and produce hydrogen gas, which will quickly ride to the top of the graduated cylinder as it is significantly less dense than any water based solution. The experimental molar volume is expected to be the same as the theoretical molar volume of any gas at STP, 22.4 L/mol, for the amount of moles in any given sample of gas is the same. Taking in account the possible sources of error and steps that could’ve been taken to improve the accuracy, we will compare the two values. Furthermore, this experiment will require factoring in the pressure of the water volume in the gaseous mixture, this can be used to calculate the actual pressure of the gas.