In the combustion of ethanol, 20.50 g of carbon dioxide gas was produced, What is the volume in mL of ethanol was used? Density of ethanol is 0.789 g/mL. C2H5OH (1) +302 (g) → 2 CO2 (g) + 3 H2O (1)
In the combustion of ethanol, 20.50 g of carbon dioxide gas was produced, What is the volume in mL of ethanol was used? Density of ethanol is 0.789 g/mL. C2H5OH (1) +302 (g) → 2 CO2 (g) + 3 H2O (1)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![**Combustion of Ethanol: Calculating Volume of Ethanol Used**
In the combustion of ethanol, 20.50 g of carbon dioxide gas was produced. What is the volume in milliliters (mL) of ethanol used? The density of ethanol is 0.789 g/mL.
The chemical equation for the combustion of ethanol is as follows:
\[ \text{C}_2\text{H}_5\text{OH} (\ell) + 3\text{O}_2 (g) \rightarrow 2\text{CO}_2 (g) + 3\text{H}_2\text{O} (\ell) \]
This equation shows that one mole of ethanol reacts with three moles of oxygen to produce two moles of carbon dioxide and three moles of water.
To find the volume of ethanol used, follow these steps:
1. **Determine the moles of CO₂ produced.**
2. **Use stoichiometry to find the moles of ethanol consumed.**
3. **Calculate the mass of ethanol used, then convert to volume using the density of ethanol.**
**Detailed Explanation:**
1. **Calculate moles of CO₂ produced:**
The molar mass of CO₂ (carbon dioxide) is 44.01 g/mol.
\[ \text{Moles of CO}_2 = \frac{20.50 \text{ g}}{44.01 \text{ g/mol}} \]
2. **Use stoichiometry to find moles of ethanol:**
From the balanced equation, 2 moles of CO₂ are produced per 1 mole of ethanol.
\[ \text{Moles of ethanol} = \frac{\text{Moles of CO}_2}{2} \]
3. **Convert moles of ethanol to mass and then to volume:**
The molar mass of ethanol (C₂H₅OH) is 46.07 g/mol.
\[ \text{Mass of ethanol} = \text{Moles of ethanol} \times 46.07 \text{ g/mol} \]
Using the density of ethanol (0.789 g/mL), convert the mass to volume.
\[ \text{Volume of ethanol} = \frac{\text{Mass of ethanol}}{0.789 \text{ g/mL}} \]
By performing these](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2cfae0b3-b761-48b0-bf7a-43df83f62bab%2F54f85548-e219-4f97-a93d-546757ce6079%2Fhi8und_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Combustion of Ethanol: Calculating Volume of Ethanol Used**
In the combustion of ethanol, 20.50 g of carbon dioxide gas was produced. What is the volume in milliliters (mL) of ethanol used? The density of ethanol is 0.789 g/mL.
The chemical equation for the combustion of ethanol is as follows:
\[ \text{C}_2\text{H}_5\text{OH} (\ell) + 3\text{O}_2 (g) \rightarrow 2\text{CO}_2 (g) + 3\text{H}_2\text{O} (\ell) \]
This equation shows that one mole of ethanol reacts with three moles of oxygen to produce two moles of carbon dioxide and three moles of water.
To find the volume of ethanol used, follow these steps:
1. **Determine the moles of CO₂ produced.**
2. **Use stoichiometry to find the moles of ethanol consumed.**
3. **Calculate the mass of ethanol used, then convert to volume using the density of ethanol.**
**Detailed Explanation:**
1. **Calculate moles of CO₂ produced:**
The molar mass of CO₂ (carbon dioxide) is 44.01 g/mol.
\[ \text{Moles of CO}_2 = \frac{20.50 \text{ g}}{44.01 \text{ g/mol}} \]
2. **Use stoichiometry to find moles of ethanol:**
From the balanced equation, 2 moles of CO₂ are produced per 1 mole of ethanol.
\[ \text{Moles of ethanol} = \frac{\text{Moles of CO}_2}{2} \]
3. **Convert moles of ethanol to mass and then to volume:**
The molar mass of ethanol (C₂H₅OH) is 46.07 g/mol.
\[ \text{Mass of ethanol} = \text{Moles of ethanol} \times 46.07 \text{ g/mol} \]
Using the density of ethanol (0.789 g/mL), convert the mass to volume.
\[ \text{Volume of ethanol} = \frac{\text{Mass of ethanol}}{0.789 \text{ g/mL}} \]
By performing these
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