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Aligned with AP Chemistry Lab #5


The ideal gas law gives an accurate description of the behavior of real gases at low pressures and at temperatures that are high relative to the boiling point. The ideal gas law is based on the assumption that the molecules experience no intermolecular forces and that the molecules occupy no volume. In reality, intermolecular forces do exist and molecules do occupy space. The extent to which these factors cause a gas to deviate from the ideal gas law at a particular temperature and pressure will determine its molecular structure. In this experiment students measure the molar volume of oxygen gas, and compare the measured value to the value predicted by the ideal gas law. A separate step leads students through the determination of the percentage KClO3 in an unknown sample. Includes materials for 15 setups.

Chemical Contents:
Potassium Chlorate
Manganese Dioxide

Additional Materials required:
1L flasks
600ml beakers
Test tubes, 16 x 150mm
Bunsen Burners
Ring stands with test tube clamps
Rubber stoppers, one and two-hole
Glass and rubber tubing


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