マグネシウムを用いたガス化学量論

Mgと塩酸の反応でモル体積を計算する

Gas Laws Intermediate (High School) 40 分 ~$8.00

目的

既知の質量のマグネシウムリボンを過剰な塩酸と反応させ、室温条件下での水素ガスのモル体積を決定する。

背景

When magnesium reacts with HCl, hydrogen gas is produced: Mg + 2HCl → MgCl₂ + H₂. By measuring the mass of Mg used and the volume of H₂ collected, the molar volume at room conditions can be calculated and compared with the theoretical value at STP (22.4 L/mol).

安全上の警告

  • HCl is corrosive
  • Hydrogen is flammable — no flames
  • Handle glassware carefully

必要なPPE

goggles gloves lab_coat

材料

  • Magnesium ribbon (0.1 g)
    Accurately weighed
  • Hydrochloric acid (HCl) (30 mL)
    2M, excess
  • Distilled water (500 mL)

器具

Eudiometer tube or graduated cylinder (50 mL) Pneumatic trough Copper wire cage Rubber stopper Analytical balance Thermometer Barometer

手順

1

Weigh a 3-4 cm strip of magnesium ribbon accurately. Record mass to 0.001 g.

3 分
2

Roll the Mg ribbon and secure it in a copper wire cage attached to a rubber stopper.

3 分
3

Fill the eudiometer tube with 2M HCl. Insert the stopper+Mg assembly, inverting the tube into the trough.

5 分 Handle acid carefully
4

Allow the reaction to complete. All the Mg should dissolve, producing H₂ gas that collects at the top.

10 分 No flames nearby
5

Equalize water levels inside and outside the tube. Read the gas volume at the meniscus.

3 分
6

Record room temperature and atmospheric pressure.

2 分
7

Correct for water vapor pressure. Calculate moles of H₂ from Mg mass. Determine molar volume.

8 分

予想される結果

0.1 g Mg = 0.00411 mol, producing 0.00411 mol H₂. At room conditions (~25°C, 1 atm), volume should be about 100 mL. Calculated molar volume at STP should be approximately 22.4 L/mol (±5%).

後片付け

Neutralize remaining HCl with NaHCO₃. Dispose down the drain. Rinse all equipment.

詳細

カテゴリ
Gas Laws
難易度
Intermediate (High School)
所要時間
40 分
推定費用
$8.00
ステップ数
7
材料
3

その他の実験

CO₂と石灰水のテスト 20 min STPでの気体のモル体積 35 min シャルルの法則（風船実験） 30 min デカルトダイバー 15 min ボイルの法則の検証 40 min 拡散速度の比較（グラハムの法則） 30 min 水素ガスの捕集 35 min 蒸気圧と沸点 45 min

Frequently Asked Questions

What is the objective of マグネシウムを用いたガス化学量論?
既知の質量のマグネシウムリボンを過剰な塩酸と反応させ、室温条件下での水素ガスのモル体積を決定する。
How difficult is マグネシウムを用いたガス化学量論?
This experiment is rated as Intermediate (High School). It takes approximately 40 minutes to complete.
What safety precautions are needed for マグネシウムを用いたガス化学量論?
Key safety precautions include: HCl is corrosive; Hydrogen is flammable — no flames; Handle glassware carefully.
What materials are needed for マグネシウムを用いたガス化学量論?
The main materials required are: Magnesium ribbon, Hydrochloric acid (HCl), Distilled water.
What results should I expect from マグネシウムを用いたガス化学量論?
0.1 g Mg = 0.00411 mol, producing 0.00411 mol H₂. At room conditions (~25°C, 1 atm), volume should be about 100 mL. Calculated molar volume at STP should be approximately 22.4 L/mol (±5%).