Place the coefficients into the underlined spaces to balance the chemical equation. Not all coefficients must be used and some may be used more than once.

Question

AgNO3 (aq) +
Zn (s)
Ag (s) +
Zn(NO3)2 (aq)
1
2
3

Answer 1

To balance the chemical equation involving silver nitrate (AgNO3), zinc (Zn), silver (Ag), and zinc nitrate (Zn(NO3)2), we can follow these steps:

1. Write the unbalanced equation: \[ \text{AgNO}_3 (aq) + \text{Zn} (s) \rightarrow \text{Ag} (s) + \text{Zn(NO}_3\text{)}_2 (aq) \]

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

   • Reactants:
     • Ag: 1 from AgNO3
     • N: 1 from AgNO3
     • O: 3 from AgNO3
     • Zn: 1 from Zn
   • Products:
     • Ag: 1 from Ag
     • N: 2 from Zn(NO3)2
     • O: 6 from Zn(NO3)2
     • Zn: 1 from Zn(NO3)2

3. It's clear that we need to balance the nitrogen and oxygen atoms. We can start by observing that we need:

   • 2 AgNO3 to provide 2 Ag and balance the nitrogen in Zn(NO3)2.

4. Now write the new equation: \[ 2\text{AgNO}_3 (aq) + \text{Zn} (s) \rightarrow 2\text{Ag} (s) + \text{Zn(NO}_3\text{)}_2 (aq) \]

5. Re-check to confirm both sides are balanced:

   • On the left side:
     • Ag: 2
     • N: 2
     • O: 6
     • Zn: 1
   • On the right side:
     • Ag: 2
     • N: 2
     • O: 6
     • Zn: 1

Both sides are now balanced.

The balanced equation is: \[ \underline{2} \text{AgNO}_3 (aq) + \underline{1} \text{Zn} (s) \rightarrow \underline{2} \text{Ag} (s) + \underline{1} \text{Zn(NO}_3\text{)}_2 (aq) \]

Fill in the blanks:

1. 2 (for AgNO3)
2. 1 (for Zn)
3. 2 (for Ag)
4. 1 (for Zn(NO3)2)

So the coefficients used are:

• 2 for AgNO3
• 1 for Zn
• 2 for Ag
• 1 for Zn(NO3)2