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The Molar Volume of a Gas

Experiment #5 from Advanced Chemistry with Vernier

Education Level
High School


In this experiment, you will determine the molar volume of a gas by conducting a chemical reaction that produces a gas, as shown in the reaction equation below.

{\text{Mg}}\left( {\text{s}} \right){\text{ }} + {\text{ 2HCl}}\left( {{\text{aq}}} \right) \to {\text{MgC}}{{\text{l}}_{\text{2}}}\left( {{\text{aq}}} \right){\text{ }} + {\text{ }}{{\text{H}}_{\text{2}}}\left( {\text{g}} \right)

You will react a known mass of solid magnesium with an excess of hydrochloric acid, in a sealed vessel, and use the pressure change to calculate molar volume at STP.


In this experiment, you will

  • Measure the gas production of a chemical reaction by a pressure change.
  • Determine the molar volume of the gas produced in the reaction.
  • Calculate the molar volume of a gas at STP.

Sensors and Equipment

This experiment features the following sensors and equipment. Additional equipment may be required.


Teaching to an educational standard? This experiment supports the standards below.

International Baccalaureate (IB) 2025/Chemistry
Structure 1.5.3—The molar volume of an ideal gas is a constant at a specific temperature and pressure.

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This experiment is #5 of Advanced Chemistry with Vernier. The experiment in the book includes student instructions as well as instructor information for set up, helpful hints, and sample graphs and data.

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