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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
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The reason the molar mass will be at 22.4L/ mol is because every gas at STP, occupies the same space a certain temperature and pressure[1]. As a result of this every gas the same molar volume, but a different density[2]. The reason all ideal gases have the same volume is because of several reasons: firstly they experience essentially no intermolecular forces, secondly they experience elastic collisions, next are able to be compressed to an extremely small volume under the right conditions and lastly their kinetic energy is directly proportional to the temperature in Kelvin, meaning if the pressure is higher, then the temperature is also higher[3]. If Mg is added to HCl, then H2 (Hydrogen gas) is created, and this gas will be at the molar volume (22.4L/ mol).

Materials Used: * Safety Goggles * Steel Wool * Ruler * Copper wire * Thermometer * Graduated Cylinder * 2 Hole Stopper * Magnesium * Large Beaker * HCL (3.0 mol/ L) * Water

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Method: 1. Measure and record the air and water temperature. 2. Prepare a copper coil using the copper wire. 3. Cut the magnesium into a few centimeters, and calculate the weight according to the weight per cm given. 4. Record the weight of that magnesium, and place it into the coil. 5. Place the coil, with the Magnesium inside of it, onto the 2-hole stopper. 6.

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