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Posted by on Sunday, October 10, 2010 at 10:36pm.

A sample of magnesium with a mass of 1.00 g is burned in oxygen to produce an oxide with a mass of 1.66 g. What is the empirical formula of the magnesium oxide produced? I know the answer is MgO. What are the steps to get that answer?

  • Chemistry - , Sunday, October 10, 2010 at 11:52pm

    Convert grams to moles.
    1.00 g Mg/ 24.3 = moles Mg

    g Osygen = 1.66-1.00 = 0.66
    moles oxygen = 0.66/16 = moles O.

    Now find the ratio of the two in and round to whole numbers. You will find 1:1 ratio.

  • Chemistry - , Monday, December 15, 2014 at 8:18pm

    DrBob222 messed up at the oxygen, it should be O2 not O. so it would be:

    Convert grams to moles.
    1.00 g Mg/ 24.3 = 0.0411... moles Mg

    g Oxygen = 1.66-1.00 = 0.66 g
    moles oxygen = 0.66/32 = 0.0206... moles O.

    Now find the ratio of the two in and round to whole numbers. You will find 2:1 ratio. (Mg2O)

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