Using Stoichiometry to Determine Gases Produced in a Reaction
Using Stoichiometry to Determine Gases Produced in a Reaction
Introduction Magnesium is a metal and is the third most commonly used metal by chemists. Some would say it is the least dense structural metal. Its lightness is often alloyed with aluminum. Magnesium is also used in racing car wheels called MAG wheels. Many car-manufacturing companies will use magnesium and aluminum because of the lightness of the metal. Both of these metals are reactive with acids. The most common acid in they react with is hydrochloric acid. In this lab, we collected a gas produced in a reaction and compared it with the volume that was actually collected to the “target volume” we calculated at the beginning of the class using stoichiometry and the Ideal Gas Law. We had to figure out what the temperature of the room was because the laboratory was not under the conditions of STP. We were given two different elements to make a reaction. The two elements were magnesium and hydrochloric acid. The balanced equation looks like this:
Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g)
To find the the predicted volume of H2, we calculated the mass of Mg needed to produce that volume.
Materials and Procedure
Thermometer
Gas collecting tube or graduated cylinder
Ruler
Balcance
Bucket or large bowl or beaker
1 or 2 hole rubber stopper
Copper wire
Magnesium ribbon
HCl, 6M
When starting this procedure make sure you are wearing the correct safety equipment.
1. Take the piece of magnesium ribbon and clean it using a piece of steel wool.
2. After cleaning the magnesium, find the mass of 30 cm of the ribbon.
3. Using stoichiometry and the ideal gas law, calculate the mass of magnesium metal needed to collect exactly 40 mL of H2 gas from the reaction given. Make sure to use current temperature and local barometric pressure.
4. Calculate the length of magnesium ribbon using the mass you found in step 3.
5. Cut the length needed of magnesium ribbon.
6. Obtain about 25 cm of copper wire
Introduction Magnesium is a metal and is the third most commonly used metal by chemists. Some would say it is the least dense structural metal. Its lightness is often alloyed with aluminum. Magnesium is also used in racing car wheels called MAG wheels. Many car-manufacturing companies will use magnesium and aluminum because of the lightness of the metal. Both of these metals are reactive with acids. The most common acid in they react with is hydrochloric acid. In this lab, we collected a gas produced in a reaction and compared it with the volume that was actually collected to the “target volume” we calculated at the beginning of the class using stoichiometry and the Ideal Gas Law. We had to figure out what the temperature of the room was because the laboratory was not under the conditions of STP. We were given two different elements to make a reaction. The two elements were magnesium and hydrochloric acid. The balanced equation looks like this:
Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g)
To find the the predicted volume of H2, we calculated the mass of Mg needed to produce that volume.
Materials and Procedure
Thermometer
Gas collecting tube or graduated cylinder
Ruler
Balcance
Bucket or large bowl or beaker
1 or 2 hole rubber stopper
Copper wire
Magnesium ribbon
HCl, 6M
When starting this procedure make sure you are wearing the correct safety equipment.
1. Take the piece of magnesium ribbon and clean it using a piece of steel wool.
2. After cleaning the magnesium, find the mass of 30 cm of the ribbon.
3. Using stoichiometry and the ideal gas law, calculate the mass of magnesium metal needed to collect exactly 40 mL of H2 gas from the reaction given. Make sure to use current temperature and local barometric pressure.
4. Calculate the length of magnesium ribbon using the mass you found in step 3.
5. Cut the length needed of magnesium ribbon.
6. Obtain about 25 cm of copper wire