When magnesium metal is burned in air (Figure 3.6), twoproducts are produced. One is magnesium oxide, MgO. Theother is the product of the reaction of Mg with molecularnitrogen, magnesium nitride. When water is added to magnesiumnitride, it reacts to form magnesium oxide and ammoniagas. (a) Based on the charge of the nitride ion (Table2.5), predict the formula of magnesium nitride. (b) Write abalanced equation for the reaction of magnesium nitridewith water. What is the driving force for this reaction? (c) Inan experiment, a piece of magnesium ribbon is burned in airin a crucible. The mass of the mixture of MgO and magnesiumnitride after burning is 0.470 g. Water is added to thecrucible, further reaction occurs, and the crucible is heated todryness until the final product is 0.486 g of MgO. What wasthe mass percentage of magnesium nitride in the mixture obtainedafter the initial burning? (d) Magnesium nitride canalso be formed by reaction of the metal with ammonia at hightemperature. Write a balanced equation for this reaction. If a6.3-g Mg ribbon reacts with 2.57 g NH31g2 and the reactiongoes to completion, which component is the limiting reactant?What mass of H21g2 is formed in the reaction? (e) Thestandard enthalpy of formation of solid magnesium nitride is-461.08 kJ>mol. Calculate the standard enthalpy change forthe reaction between magnesium metal and ammonia gas.
When magnesium metal is burned in air (Figure 3.6), two
products are produced. One is magnesium oxide, MgO. The
other is the product of the reaction of Mg with molecular
nitrogen, magnesium nitride. When water is added to magnesium
nitride, it reacts to form magnesium oxide and ammonia
gas. (a) Based on the charge of the nitride ion (Table
2.5), predict the formula of magnesium nitride. (b) Write a
balanced equation for the reaction of magnesium nitride
with water. What is the driving force for this reaction? (c) In
an experiment, a piece of magnesium ribbon is burned in air
in a crucible. The mass of the mixture of MgO and magnesium
nitride after burning is 0.470 g. Water is added to thecrucible, further reaction occurs, and the crucible is heated to
dryness until the final product is 0.486 g of MgO. What was
the mass percentage of magnesium nitride in the mixture obtained
after the initial burning? (d) Magnesium nitride can
also be formed by reaction of the metal with ammonia at high
temperature. Write a balanced equation for this reaction. If a
6.3-g Mg ribbon reacts with 2.57 g NH31g2 and the reaction
goes to completion, which component is the limiting reactant?
What mass of H21g2 is formed in the reaction? (e) The
standard enthalpy of formation of solid magnesium nitride is
-461.08 kJ>mol. Calculate the standard enthalpy change for
the reaction between magnesium metal and ammonia gas.
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