1. In a certain compound of copper and oxygen, CuxOy, we find that a sample weighing 0.6349 g contains 0.5639 g of Cu. What is the mole ratio (number of moles Cu/number of moles O) in the sample? Write the resulting Empirical Formula.
1. In a certain compound of copper and oxygen, CuxOy, we find that a sample weighing 0.6349 g contains 0.5639 g of Cu. What is the mole ratio (number of moles Cu/number of moles O) in the sample? Write the resulting Empirical Formula.
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![### Determining the Empirical Formula of a Copper and Oxygen Compound
**Problem Statement:**
1. In a certain compound of copper and oxygen, \( \text{Cu}_x\text{O}_y \), we find that a sample weighing 0.6349 g contains 0.5639 g of Cu. What is the mole ratio (number of moles Cu/number of moles O) in the sample? Write the resulting Empirical Formula.
**Solution:**
To determine the empirical formula of the compound, follow these steps:
1. **Determine the Mass of Each Element:**
- Mass of copper (Cu) = 0.5639 g
- Mass of oxygen (O) = Total mass - Mass of copper
\[
\text{Mass of oxygen} = 0.6349 \text{ g} - 0.5639 \text{ g} = 0.0710 \text{ g}
\]
2. **Calculate the Number of Moles of Each Element:**
- For copper (Cu):
\[
\text{Moles of Cu} = \frac{\text{Mass of Cu}}{\text{Atomic mass of Cu}} = \frac{0.5639 \text{ g}}{63.55 \text{ g/mol}} \approx 0.00887 \text{ mol}
\]
- For oxygen (O):
\[
\text{Moles of O} = \frac{\text{Mass of O}}{\text{Atomic mass of O}} = \frac{0.0710 \text{ g}}{16.00 \text{ g/mol}} \approx 0.00444 \text{ mol}
\]
3. **Determine the Mole Ratio:**
- Find the simplest ratio by dividing each number of moles by the smaller value:
\[
\text{Ratio of Cu} = \frac{0.00887}{0.00444} \approx 2
\]
\[
\text{Ratio of O} = \frac{0.00444}{0.00444} = 1
\]
4. **Write the Empirical Formula:**
- Using the mole ratios, the empirical formula is \( \text{Cu}_2\text{O} \).
By following these steps, you](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6ae95cc5-a0cd-43b0-8331-9678c9dacca0%2F9394ff95-361b-4fdc-8d94-e44a0b9b4099%2Fkvuwpo.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining the Empirical Formula of a Copper and Oxygen Compound
**Problem Statement:**
1. In a certain compound of copper and oxygen, \( \text{Cu}_x\text{O}_y \), we find that a sample weighing 0.6349 g contains 0.5639 g of Cu. What is the mole ratio (number of moles Cu/number of moles O) in the sample? Write the resulting Empirical Formula.
**Solution:**
To determine the empirical formula of the compound, follow these steps:
1. **Determine the Mass of Each Element:**
- Mass of copper (Cu) = 0.5639 g
- Mass of oxygen (O) = Total mass - Mass of copper
\[
\text{Mass of oxygen} = 0.6349 \text{ g} - 0.5639 \text{ g} = 0.0710 \text{ g}
\]
2. **Calculate the Number of Moles of Each Element:**
- For copper (Cu):
\[
\text{Moles of Cu} = \frac{\text{Mass of Cu}}{\text{Atomic mass of Cu}} = \frac{0.5639 \text{ g}}{63.55 \text{ g/mol}} \approx 0.00887 \text{ mol}
\]
- For oxygen (O):
\[
\text{Moles of O} = \frac{\text{Mass of O}}{\text{Atomic mass of O}} = \frac{0.0710 \text{ g}}{16.00 \text{ g/mol}} \approx 0.00444 \text{ mol}
\]
3. **Determine the Mole Ratio:**
- Find the simplest ratio by dividing each number of moles by the smaller value:
\[
\text{Ratio of Cu} = \frac{0.00887}{0.00444} \approx 2
\]
\[
\text{Ratio of O} = \frac{0.00444}{0.00444} = 1
\]
4. **Write the Empirical Formula:**
- Using the mole ratios, the empirical formula is \( \text{Cu}_2\text{O} \).
By following these steps, you
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