1. An unknown oxide of mercury decomposes when heated to form mercury metal and
oxygen gas (O
2). When a 1.048 g sample of this unknown is heated, 0.971 g of mercury remains.
a. Calculate the moles of mercury and moles of oxygen in the compound.
b. What is the empirical formula of this oxide?
2. a) A side reaction in today’s experiment occurs between some of the magnesium and
the nitrogen gas, N
2. Write a balanced chemical equation for this reaction. b) The magnesium nitride can be converted to magnesium oxide by the addition of
water. Write a balanced chemical equation for this reaction.
3. Suppose 1.087g of magnesium is heated in air. What is the theoretical amount of
magnesium oxide that should be produced?
4. Calculate the percent by mass of molybdenum and sulfur in Mo2S5.
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