Question

When potassium chloride and lead ($II$) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation?

• A. $Pb{Cl}_{\left(s\right)}$
• B. ${Pb}_2{Cl}_{\left(s\right)}$
• C. $K{NO}_{3\left(aq\right)}$
• D. $2K{NO}_{3\left(aq\right)}$
• E. $2K{Cl}_{2\left(s\right)}$

Answer 1

The correct option is D $2K{NO}_{3\left(aq\right)}$

Rules for solving or balancing a chemical equation:-

1. Write an unbalanced equation.

2. Assign oxidation number for each atom.

3. Separate out reactions into two half reactions.

4. Balance all other atoms except $H$ and $O$ in each half reaction.

5. Balance the hydrogen by $H^{+}$ or $O{H}^{-}$ .

6. Balance the oxygen atoms by $H_{2}O$.

7. Make electron gain equivalent to electron loss in the half reactions by multiplying them with respective numbers.

8. Add and simplify the half reactions together.

9. Check for elements and charges are balanced.

$\underset{\left(PotassiumChloride\right)}{2KCl}+\underset{\left(Lead\right(II\left)Nitrate\right)}{Pb(N{O}_3{)}_2}\stackrel{(aq.)}{\to }\underset{\left(PotassiumNitrate\right)}{2KN{O}_3}+\underset{\left(Lead\right(II\left)Chloride\right)}{PbC{l}_2}$

This is the balanced equation, when potassium chloride reacts with lead nitrate in an aqueous solution.