Compute the moles of mercury and moles of oxygen

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Reference no: EM13675793

An unknown oxide of mercury decomposes while heated to form mercury metal and oxygen gas. While a 1.048 g sample of this unknown is heated, 0.971 g of mercury remains.

a. Compute the moles of mercury and moles of oxygen in the compound.

b. Explain what is the empirical formula of this oxide?

2. A side reaction in today's experiment takes place between some of the magnesium and the nitrogen gas, N2.

a. State a balanced chemical equation for this reaction.

b. If the magnesium nitride can be converted to magnesium oxide by the addition of water. State a balanced chemical equation for this reaction.

Reference no: EM13675793

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