A particular beer is 6.50% ethanol by volume (C₂H₂O). If a single bottle of beer contains 750.0 mL of beer, what mass, in g of ethanol (C₂H₂O), is present in the bottle? The density of ethanol is 0.789 g ethanol/mL ethanol
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Please set up the answer the correct way. I am having a hard time with putting the units in the correct spots.
![### Problem Statement
A particular beer is **6.50 % ethanol by volume (C₂H₆O)**. If a single bottle of beer contains **750.0 mL of beer**, what mass, in **g of ethanol (C₂H₆O)**, is present in the bottle? The density of ethanol is **0.789 g ethanol/mL ethanol**.
### Diagram Explanation
#### Equation Setup:
The diagram helps set up the calculation as follows:
**Starting Amount:**
- Initial volume of beer available, given as 750.0 mL.
**Calculation Formula:**
The diagram provides a structure to solve the problem step-by-step visually, using multiplication and unit conversions.
**Given Variables:**
- Percentage of ethanol by volume in beer: 6.50%
- Volume of the beer: 750.0 mL
- Density of ethanol: 0.789 g ethanol/mL ethanol
#### Detailed Steps:
1. **Determine Volume of Ethanol:**
\[ \text{Volume of ethanol} = \text{Volume of beer} \times \left( \frac{\text{\% ethanol}}{100} \right) \]
Where:
- Volume of beer is 750.0 mL
- Percentage of ethanol by volume is 6.50%
- Hence, Volume of ethanol is \( 750.0 \, \text{mL} \times \left( \frac{6.50}{100} \right) = 48.75 \, \text{mL ethanol} \)
2. **Convert Volume of Ethanol to Mass of Ethanol:**
\[ \text{Mass of ethanol} = \text{Volume of ethanol} \times \text{Density of ethanol} \]
- Volume of ethanol is 48.75 mL
- Density of ethanol is 0.789 g/mL
- Hence, Mass of ethanol is \( 48.75 \, \text{mL ethanol} \times 0.789 \, \text{g/mL} \)
3. **Calculation:**
\[ \text{Mass of ethanol} = 48.75 \, \text{mL ethanol} \times 0.789 \, \text{g/mL} = 38.45 \, \text{g ethanol} \]
### Conclusion](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffbb15d99-77db-4308-835f-20d2902f98e0%2F37f09111-f233-4c27-9ed1-ca92ed560d77%2Fqjg8z0l_processed.png&w=3840&q=75)
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