1) CaC2 + H2O → Ca(OH)2 + C2H2

a. Balanced equation:

b. If you have 5.50 mol of CaC2, how much (grams) C2H2 do you get?

c. How many moles of water are needed when 65.0g of CaC2 reacts?

Let's address the questions one by one.

### a. Balanced equation:

The given equation is:

\[
\text{CaC}_2 + \text{H}_2\text{O} \rightarrow \text{Ca(OH)}_2 + \text{C}_2\text{H}_2
\]

Balancing the equation, we get:

\[
\text{CaC}_2 + 2\text{H}_2\text{O} \rightarrow \text{Ca(OH)}_2 + \text{C}_2\text{H}_2
\]

### b. If you have 5.50 mol of CaC2, how much (grams) C2H2 do you get?

From the balanced equation, 1 mole of **CaC₂** produces 1 mole of **C₂H₂** (acetylene).

- Moles of CaC₂ = 5.50 mol
- Molar mass of C₂H₂ = (2 × 12.01 g/mol for Carbon) + (2 × 1.008 g/mol for Hydrogen) = 26.04 g/mol

So, the mass of C₂H₂ produced can be calculated as:

\[
\text{Mass of C}_2\text{H}_2 = \text{Moles of C}_2\text{H}_2 \times \text{Molar mass of C}_2\text{H}_2
\]

\[
\text{Mass of C}_2\text{H}_2 = 5.50 \, \text{mol} \times 26.04 \, \text{g/mol} = 143.22 \, \text{g}
\]

### c. How many moles of water are needed when 65.0 g of CaC2 reacts?

First, find the molar mass of **CaC₂**:
\[
\text{Molar mass of CaC}_2 = (1 \times 40.08 \, \text{g/mol for Calcium}) + (2 \times 12.01 \, \text{g/mol for Carbon}) = 64.10 \, \text{g/mol}
\]

Now, calculate the moles of **CaC₂** in 65.0 g:

\[
\text{Moles of CaC}_2 = \frac{65.0 \, \text{g}}{64.10 \, \text{g/mol}} = 1.014 \, \text{mol}
\]

From the balanced equation, 1 mole of **CaC₂** requires 2 moles of **H₂O**. Therefore, the moles of **H₂O** needed are:

\[
\text{Moles of H}_2\text{O} = 2 \times 1.014 \, \text{mol} = 2.028 \, \text{mol}
\]

---

### Summary of Answers:

a. **Balanced Equation**:  
\[
\text{CaC}_2 + 2\text{H}_2\text{O} \rightarrow \text{Ca(OH)}_2 + \text{C}_2\text{H}_2
\]

b. **Mass of C₂H₂ from 5.50 mol of CaC₂**:  
\[
143.22 \, \text{g}
\]

c. **Moles of H₂O needed for 65.0 g of CaC₂**:  
\[
2.028 \, \text{mol}
\]

---

Would you like any details or further clarification?

Here are some related questions for further practice:

1. How much (grams) of Ca(OH)₂ is produced from 5.50 mol of CaC₂?
2. What is the mass of water required to fully react with 65.0 g of CaC₂?
3. How many moles of Ca(OH)₂ are produced when 0.500 mol of CaC₂ reacts?
4. If 2.00 mol of H₂O is used, how many grams of C₂H₂ are formed?
5. How much (grams) CaC₂ is required to produce 50.0 g of C₂H₂?

**Tip**: Always ensure your chemical equations are balanced before solving stoichiometry problems!

Learn how to balance the equation CaC2 + H2O → Ca(OH)2 + C2H2 and perform stoichiometric calculations. Find out how many grams of C2H2 are produced from 5.50 mol of CaC2 and how many moles of water are needed for 65.0g of CaC2. Suitable for Grades 10-12.

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