A particular beer is 6.50 % ethanol by volume (C₂H₆O). If a single bottle of beer contain 750.0 mL of beer, what mass, in g of ethanol (C₂H₆O), is present in the bottle? The density of ethanol is 0.789g ethanol/mL ethanol. Can this be solved to fill in the blanks and only with the numbers given?
A particular beer is 6.50 % ethanol by volume (C₂H₆O). If a single bottle of beer contain 750.0 mL of beer, what mass, in g of ethanol (C₂H₆O), is present in the bottle? The density of ethanol is 0.789g ethanol/mL ethanol. Can this be solved to fill in the blanks and only with the numbers given?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A particular beer is 6.50 % ethanol by volume (C₂H₆O). If a single bottle of beer contain 750.0 mL of beer, what mass, in g of ethanol (C₂H₆O), is present in the bottle? The density of ethanol is 0.789g ethanol/mL ethanol.
Can this be solved to fill in the blanks and only with the numbers given?
![### Question 5 of 25
A particular beer is **6.50% ethanol by volume** (C₂H₅OH). If a single bottle of beer contains **750.0 mL of beer**, what mass, in grams, of ethanol (C₂H₅OH) is present in the bottle? The density of ethanol is **0.789 g ethanol/mL ethanol**.
#### Given:
- **6.50% ethanol by volume**
- **750.0 mL of beer**
- **Density of ethanol: 0.789 g/mL**
#### Calculation Steps:
1. **Determine the volume of ethanol in the beer**:
\[
\text{Volume of ethanol} = \left(\frac{6.50}{100}\right) \times 750.0\,\text{mL}
\]
2. **Calculate the mass of ethanol using its density**:
\[
\text{Mass of ethanol} = \text{Volume of ethanol} \times 0.789\,\text{g/mL}
\]
#### Diagram/Graph Description:
- The diagram displays three boxes signifying the calculation process:
- The first box indicates the starting amount: **6.50**
- The second box: \[
\begin{array}{c}
750.0\, \, \text{mL beer}\\
\left(\frac{\text{ethanol volume percentage}}{100}\right)
\end{array}
\]
- The third box: \[
\begin{array}{c}
\left(\text{ethanol volume}\right) \times 0.789\, \, \text{g/mL}
\end{array}
\]
The interface also includes a numerical keypad and function buttons for adding, deleting, and inserting answers.
This question requires understanding of the volume-to-mass conversion and utilization of the density formula. The provided calculation steps will assist students in achieving the correct answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F155609b6-c9e3-478d-91a5-0673fb3bee9a%2Faf85f696-b360-42e6-85b8-e07108b35927%2Fes1ogr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question 5 of 25
A particular beer is **6.50% ethanol by volume** (C₂H₅OH). If a single bottle of beer contains **750.0 mL of beer**, what mass, in grams, of ethanol (C₂H₅OH) is present in the bottle? The density of ethanol is **0.789 g ethanol/mL ethanol**.
#### Given:
- **6.50% ethanol by volume**
- **750.0 mL of beer**
- **Density of ethanol: 0.789 g/mL**
#### Calculation Steps:
1. **Determine the volume of ethanol in the beer**:
\[
\text{Volume of ethanol} = \left(\frac{6.50}{100}\right) \times 750.0\,\text{mL}
\]
2. **Calculate the mass of ethanol using its density**:
\[
\text{Mass of ethanol} = \text{Volume of ethanol} \times 0.789\,\text{g/mL}
\]
#### Diagram/Graph Description:
- The diagram displays three boxes signifying the calculation process:
- The first box indicates the starting amount: **6.50**
- The second box: \[
\begin{array}{c}
750.0\, \, \text{mL beer}\\
\left(\frac{\text{ethanol volume percentage}}{100}\right)
\end{array}
\]
- The third box: \[
\begin{array}{c}
\left(\text{ethanol volume}\right) \times 0.789\, \, \text{g/mL}
\end{array}
\]
The interface also includes a numerical keypad and function buttons for adding, deleting, and inserting answers.
This question requires understanding of the volume-to-mass conversion and utilization of the density formula. The provided calculation steps will assist students in achieving the correct answer.
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