Whether or not the reaction above can occur and result in an actual chemical change, we can write and balance an equation. Use the drop downs to add the correct coefficients to balance the equation. (4 points)

Question

Fe(OH)2
+
Mn
→
Mn(OH)4
+
Fe

Answer 1

To balance the equation given:

Unbalanced equation: \[ \text{Fe(OH)}_2 + \text{Mn} \rightarrow \text{Mn(OH)}_4 + \text{Fe} \]

Let's break down the process of balancing the equation:

1. Count the number of each type of atom on both sides:

   • Reactants:

     • Fe: 1
     • O: 2 (from 2 OH groups)
     • H: 2 (from 2 OH groups)
     • Mn: 1

   • Products:

     • Fe: 1
     • O: 4 (from 4 OH groups)
     • H: 4 (from 4 OH groups)
     • Mn: 1

2. Balance the hydroxide ions (OH) first. Notice that there are 2 OH groups on the left and 4 OH groups on the right. To balance the OH groups, we can add a coefficient of 2 in front of Fe(OH)2 on the left side.

Now the equation looks like: \[ 2 \text{Fe(OH)}_2 + \text{Mn} \rightarrow \text{Mn(OH)}_4 + 2 \text{Fe} \]

3. Count the number of each type of atom again:

   • Reactants:

     • Fe: 2
     • O: 4 (from 2 × 2 OH)
     • H: 4 (from 2 × 2 OH)
     • Mn: 1

   • Products:

     • Fe: 2
     • O: 4 (from 4 OH groups)
     • H: 4 (from 4 OH groups)
     • Mn: 1

Now both sides are balanced.

Final balanced equation: \[ 2 \text{Fe(OH)}_2 + 1 \text{Mn} \rightarrow 1 \text{Mn(OH)}_4 + 2 \text{Fe} \]

In the drop-downs:

• Fe(OH)2: 2
• Mn: 1
• Mn(OH)4: 1
• Fe: 2

So, the balanced equation has:

• Coefficient for Fe(OH)2: 2
• Coefficient for Mn: 1
• Coefficient for Mn(OH)4: 1
• Coefficient for Fe: 2