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Quantitative and Qualitative Reactions of Active Metals

  • Page ID
    221977
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    Chemical Concepts Demonstrated

    • Reactions of metals
    • Concept of equivalent weight
    • Stoichiometry

    Demonstration

    Three balloons are attached to three bottles as shown in the picture.
    • The1st balloon contains a sample of sodium metal and is attached to a bottle containing water.
    • The 2nd balloon contains a sample of magnesium metal and is attached to a bottle containing HCl.
    • The 3rd balloon contains a sample of aluminum metal and is attached to a bottle containing HCl.
    quan.gif

    The samples are then dropped into their bottles.

    Observations

    Although the same amount of metal was used in each trial, the three balloons contain different volumes of H2 gas. In fact, there is an approximate 1:2:3 ratio with respect to the resulting sizes of the balloons.

    Explanation (including important chemical equations)

    2 Na (s) + 2 H2O (l) ---> 1 H2 (g) + 2 NaOH

    2 Mg (s) + 4 HCl (l) ----> 2 H2 (g) + 2 MgCl2

    2 Al (s) + 6 HCl (l) ----> 3 H2 (g) + 2 AlCl3

    The balanced chemical equations show that the stoichiometry of the three reactions is different. The molar ratios of metal to hydrogen gas indicate that the aluminum metal will produce the most gas, then magnesium, and finally sodium.

    Contributors


    Quantitative and Qualitative Reactions of Active Metals is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.

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