30. In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.

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Can anyone explain step by step (in details)how did we get the balanced equation?
**Experiment 30: Magnesium Oxidation in Air**

In a common laboratory experiment, magnesium metal is heated in the presence of air to produce magnesium oxide (MgO). Magnesium oxide is a white solid, but during the experiment, it may appear gray due to the formation of small amounts of magnesium nitride (Mg₃N₂), as some magnesium reacts with nitrogen. 

**Task:** Write a balanced equation for each reaction.

**Solution:**

1. **Formation of Magnesium Oxide:**
   \[
   2\text{Mg}(s) + \text{O}_2(g) \rightarrow 2\text{MgO}(s)
   \]

2. **Formation of Magnesium Nitride:**
   \[
   3\text{Mg}(s) + \text{N}_2(g) \rightarrow \text{Mg}_3\text{N}_2(s)
   \]

These reactions illustrate the conversion of magnesium in air, combining with oxygen and nitrogen to form different compounds.
Transcribed Image Text:**Experiment 30: Magnesium Oxidation in Air** In a common laboratory experiment, magnesium metal is heated in the presence of air to produce magnesium oxide (MgO). Magnesium oxide is a white solid, but during the experiment, it may appear gray due to the formation of small amounts of magnesium nitride (Mg₃N₂), as some magnesium reacts with nitrogen. **Task:** Write a balanced equation for each reaction. **Solution:** 1. **Formation of Magnesium Oxide:** \[ 2\text{Mg}(s) + \text{O}_2(g) \rightarrow 2\text{MgO}(s) \] 2. **Formation of Magnesium Nitride:** \[ 3\text{Mg}(s) + \text{N}_2(g) \rightarrow \text{Mg}_3\text{N}_2(s) \] These reactions illustrate the conversion of magnesium in air, combining with oxygen and nitrogen to form different compounds.
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