Balancing Equations Worksheet Solutions 1 | StudyX - Free Printable

The provided image shows a "Balancing Equations Worksheet - Solutions" with balanced chemical equations. Below, I will explain the process of balancing chemical equations and verify the solutions for a few selected examples.

Steps to Balance Chemical Equations:

1. Write the Unbalanced Equation: Start with the given reactants and products.
2. Count the Atoms: Count the number of atoms of each element on both sides of the equation.
3. Balance Elements One by One:
- Start with elements that appear in only one compound on each side.
- Use coefficients (numbers placed in front of formulas) to balance the equation.
- Avoid changing subscripts, as this would alter the compounds.
4. Check Your Work: Ensure that the number of atoms of each element is the same on both sides of the equation.
5. Verify the Equation: Double-check to ensure it is balanced.

Verification of Selected Examples:

#### Example 1:
\[
\text{H}_3\text{PO}_4 + \text{KOH} \rightarrow \text{K}_3\text{PO}_4 + \text{H}_2\text{O}
\]
- Reactants:
- H: 3 (from H₃PO₄)
- P: 1 (from H₃PO₄)
- O: 4 + 1 = 5 (from H₃PO₄ and KOH)
- K: 1 (from KOH)
- Products:
- K: 3 (from K₃PO₄)
- P: 1 (from K₃PO₄)
- O: 4 + 1 = 5 (from K₃PO₄ and H₂O)
- H: 2 (from H₂O)

To balance:
- We need 3 K atoms on the left side, so add a coefficient of 3 to KOH.
- This gives us 3 H atoms from 3 KOH molecules, which balances the H atoms when combined with H₃PO₄.
- The equation becomes:
\[
\text{H}_3\text{PO}_4 + 3\text{KOH} \rightarrow \text{K}_3\text{PO}_4 + 3\text{H}_2\text{O}
\]

#### Example 2:
\[
\text{K} + \text{B}_2\text{O}_3 \rightarrow \text{K}_2\text{O} + \text{B}
\]
- Reactants:
- K: 1
- B: 2
- O: 3
- Products:
- K: 2
- B: 1
- O: 1

To balance:
- Add a coefficient of 6 to K to balance the K atoms.
- Add a coefficient of 3 to K₂O to balance the K atoms.
- Add a coefficient of 2 to B to balance the B atoms.
- The equation becomes:
\[
6\text{K} + \text{B}_2\text{O}_3 \rightarrow 3\text{K}_2\text{O} + 2\text{B}
\]

#### Example 3:
\[
\text{Na} + \text{NaNO}_3 \rightarrow \text{Na}_2\text{O} + \text{N}_2
\]
- Reactants:
- Na: 1 + 1 = 2
- N: 1
- O: 3
- Products:
- Na: 2
- N: 2
- O: 1

To balance:
- Add a coefficient of 10 to Na to balance the Na atoms.
- Add a coefficient of 2 to NaNO₃ to balance the N atoms.
- Add a coefficient of 6 to Na₂O to balance the O atoms.
- The equation becomes:
\[
10\text{Na} + 2\text{NaNO}_3 \rightarrow 6\text{Na}_2\text{O} + \text{N}_2
\]

#### Example 4:
\[
\text{C} + \text{S}_8 \rightarrow \text{CS}_2
\]
- Reactants:
- C: 1
- S: 8
- Products:
- C: 1
- S: 2

To balance:
- Add a coefficient of 4 to C to balance the C atoms.
- Add a coefficient of 4 to CS₂ to balance the S atoms.
- The equation becomes:
\[
4\text{C} + \text{S}_8 \rightarrow 4\text{CS}_2
\]

Final Answer:

The provided solutions in the image are correct. Each equation is balanced with the appropriate coefficients.

\boxed{\text{The solutions are correct.}}