Chemistry 1 Mole of Gas

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Name of the Student:…………………Date:…………..

What is the volume of 1 mole of hydrogen gas?
One mole of any gas occupies the same volume when measured under the same conditions of temperature and pressure. In this experiment you will calculate the volume of 1 mole of hydrogen at room temperature and pressure.

Intended lesson outcomes
By the end of this practical you should be able to:
• further develop skills in manipulating apparatus and accurate measurement; • use the mole concept;
• calculate the molar volume at room temperature and pressure.

Background information
Magnesium reacts with acid to give a salt and water.

Question
1 Write the word and balanced equation for the reaction of magnesium with dilute Hydrochloric acid.

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If the mass of magnesium is measured, then the moles of magnesium can be calculated. Once this amount is known, you can use the equation you have written in Question 1 to Calculate the moles of hydrogen that are produced. If the volume of this amount of hydrogen is measured, then you can calculate the volume of 1 mole, also known as the molar volume.

Safety
[pic]

Procedure
1. Clean a piece of magnesium ribbon about 3.5 cm long then weigh it accurately. This should weigh between 0.02 g and 0.04 g; if not, adjust the length of magnesium until it does.
2. Place about 30 cm3 1M hydrochloric acid in the burette and top this up to 50 cm3 with water.
3. Push the magnesium into the top of the burette, above the liquid level, so that it is held by its own tension (see Fig. 5.1).

4. Add 50 cm3 of water to a crystallizing dish.
5. Quickly invert the burette into the water. Provided you do this quickly and carefully, you will lose very little of the liquid in the burette. The liquid level should be on the graduated scale. If it is not, open the tap for a moment to allow the level to drop. Record the burette reading.

Observation Table
[pic]
Figure 5.1
6. Clamp the...
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