Answer :
Certainly! Let’s go through the steps to write and balance the chemical equation for the formation of magnesium nitride [tex]\((Mg_3N_2)\)[/tex] from its elements.
### Step 1: Write the Unbalanced Equation
First, we need to write the unbalanced equation using the elemental forms of magnesium (Mg) and nitrogen (N[tex]\(_2\)[/tex]).
[tex]\[ \text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2\][/tex]
### Step 2: Balance Magnesium (Mg) Atoms
In the unbalanced equation, we have 3 magnesium (Mg) atoms on the right side within [tex]\( \text{Mg}_3\text{N}_2 \)[/tex], but only 1 magnesium atom on the left side. To balance the magnesium atoms, we place a coefficient of 3 in front of Mg on the reactant side.
[tex]\[ 3\text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2\][/tex]
### Step 3: Balance Nitrogen (N) Atoms
Next, let’s consider the nitrogen (N) atoms. On the left side, we have [tex]\( \text{N}_2 \)[/tex], which consists of 2 nitrogen atoms. On the right side, within [tex]\( \text{Mg}_3\text{N}_2 \)[/tex], we also have 2 nitrogen atoms. Therefore, the number of nitrogen atoms is already balanced, and we do not need to change the coefficients for the nitrogen atoms.
### Step 4: Check the Balance
Finally, let’s check our balanced equation to ensure both sides have the same number of each type of atom.
- Magnesium (Mg): 3 atoms on the left, 3 atoms on the right (in [tex]\( \text{Mg}_3\text{N}_2 \)[/tex])
- Nitrogen (N): 2 atoms on the left (in [tex]\( \text{N}_2 \)[/tex]), 2 atoms on the right (in [tex]\( \text{Mg}_3\text{N}_2 \)[/tex])
Both sides of the equation now have the same number of magnesium and nitrogen atoms, so the equation is balanced.
### Balanced Equation
The balanced chemical equation for the formation of magnesium nitride is:
[tex]\[ 3\text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2 \][/tex]
### Step 1: Write the Unbalanced Equation
First, we need to write the unbalanced equation using the elemental forms of magnesium (Mg) and nitrogen (N[tex]\(_2\)[/tex]).
[tex]\[ \text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2\][/tex]
### Step 2: Balance Magnesium (Mg) Atoms
In the unbalanced equation, we have 3 magnesium (Mg) atoms on the right side within [tex]\( \text{Mg}_3\text{N}_2 \)[/tex], but only 1 magnesium atom on the left side. To balance the magnesium atoms, we place a coefficient of 3 in front of Mg on the reactant side.
[tex]\[ 3\text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2\][/tex]
### Step 3: Balance Nitrogen (N) Atoms
Next, let’s consider the nitrogen (N) atoms. On the left side, we have [tex]\( \text{N}_2 \)[/tex], which consists of 2 nitrogen atoms. On the right side, within [tex]\( \text{Mg}_3\text{N}_2 \)[/tex], we also have 2 nitrogen atoms. Therefore, the number of nitrogen atoms is already balanced, and we do not need to change the coefficients for the nitrogen atoms.
### Step 4: Check the Balance
Finally, let’s check our balanced equation to ensure both sides have the same number of each type of atom.
- Magnesium (Mg): 3 atoms on the left, 3 atoms on the right (in [tex]\( \text{Mg}_3\text{N}_2 \)[/tex])
- Nitrogen (N): 2 atoms on the left (in [tex]\( \text{N}_2 \)[/tex]), 2 atoms on the right (in [tex]\( \text{Mg}_3\text{N}_2 \)[/tex])
Both sides of the equation now have the same number of magnesium and nitrogen atoms, so the equation is balanced.
### Balanced Equation
The balanced chemical equation for the formation of magnesium nitride is:
[tex]\[ 3\text{Mg} + \text{N}_2 \rightarrow \text{Mg}_3\text{N}_2 \][/tex]
