**Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:**

**CaO(s)+H2O(l)⟶Ca(OH)2(s)**

**In a particular experiment, a 1.50 g sample of CaO is reacted with excess water and 1.48 g of Ca(OH)2 is recovered.**

(Ch. 3) What is the ***percent yield (in %)*** in this experiment?

To find the percent yield, we need to follow these steps:

### Step 1: Write the balanced chemical equation.
The reaction is already given:
\[
\text{CaO (s)} + \text{H}_2\text{O (l)} \rightarrow \text{Ca(OH)}_2\text{(s)}
\]
This equation is balanced as written.

### Step 2: Calculate the molar masses.
- Molar mass of \(\text{CaO}\) = 40.08 g/mol (Ca) + 16.00 g/mol (O) = 56.08 g/mol
- Molar mass of \(\text{Ca(OH)}_2\) = 40.08 g/mol (Ca) + 2(16.00 g/mol O) + 2(1.008 g/mol H) = 74.10 g/mol

### Step 3: Calculate the theoretical yield.
We start with a 1.50 g sample of CaO. First, convert grams of \(\text{CaO}\) to moles:
\[
\text{Moles of CaO} = \frac{1.50 \text{ g}}{56.08 \text{ g/mol}} \approx 0.02675 \text{ moles}
\]

Since the stoichiometric ratio between CaO and Ca(OH)\(_2\) is 1:1, the moles of Ca(OH)\(_2\) produced will also be 0.02675 moles.

Now, calculate the theoretical mass of Ca(OH)\(_2\):
\[
\text{Mass of Ca(OH)}_2 = 0.02675 \text{ moles} \times 74.10 \text{ g/mol} \approx 1.982 \text{ g}
\]

### Step 4: Calculate the percent yield.
Percent yield is calculated as:
\[
\text{Percent yield} = \left(\frac{\text{Actual yield}}{\text{Theoretical yield}}\right) \times 100
\]

The actual yield of \(\text{Ca(OH)}_2\) is given as 1.48 g. Therefore:
\[
\text{Percent yield} = \left(\frac{1.48 \text{ g}}{1.982 \text{ g}}\right) \times 100 \approx 74.7\%
\]

### Final Answer:
The percent yield of \(\text{Ca(OH)}_2\) in this experiment is approximately **74.7%**.

---

Would you like more details on any step or have any questions?

Here are 5 related questions for further exploration:
1. How is theoretical yield calculated for a reaction?
2. What factors can cause the percent yield to be less than 100%?
3. What is the significance of using excess water in this reaction?
4. How can side reactions affect the actual yield in chemical reactions?
5. How would the percent yield change if less product was recovered?

**Tip:** When calculating percent yield, always ensure that your units (grams, moles) are consistent throughout the calculation!

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:

CaO(s) + H2O(l) ⟶ Ca(OH)2(s)

In a particular experiment, a 1.50 g sample of CaO is reacted with excess water and 1.48 g of Ca(OH)2 is recovered. What is the percent yield (in %) in this experiment?

Learn how to calculate the percent yield for the reaction between calcium oxide (CaO) and water to form calcium hydroxide (Ca(OH)2). This example includes detailed stoichiometric calculations and step-by-step guidance for finding the theoretical and actual yields. Suitable for high school chemistry students in Grades 10-12.

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