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The problem asks to calculate the moles of oxygen (O₂) needed to produce 1.0 mol of water (H₂O) in a reaction involving ethanol (C₂H₅OH) and oxygen.

The chemical equation for this reaction is:

\[
\text{C₂H₅OH} + 3 \text{O₂} \rightarrow 2 \text{CO₂} + 3 \text{H₂O}
\]

From the balanced equation, we see that for every 3 moles of oxygen gas (O₂), 3 moles of water (H₂O) are produced. Therefore, the ratio of oxygen to water is 1:1.

### Steps:
1. The problem asks for the moles of oxygen required to produce 1.0 mol of water.
2. Since the ratio is 1:1, the moles of oxygen required is also 1.0 mol.

Thus, the moles of oxygen needed to produce 1.0 mol of water is **1.0 mol**.

Would you like more details or explanations on any part? Here are some related questions:

1. How do you balance chemical equations like the one used here?
2. What is the role of oxygen in the combustion of ethanol?
3. How can we calculate the mass of oxygen gas needed for the reaction?
4. What other products are formed during the combustion of ethanol?
5. How do significant figures affect the calculation in this reaction?

**Tip**: Always ensure your chemical equation is balanced before doing any stoichiometric calculations!

Wine goes bad soon after opening because the ethanol (C₂H₅OH) dissolved in it reacts with oxygen (O₂) gas to form water and aqueous acetic acid (CH₃COOH), the main ingredient in vinegar. Calculate the moles of oxygen needed to produce 1.0 mol of water. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

Learn how to calculate the moles of oxygen (O₂) needed to produce 1.0 mol of water in a chemical reaction involving ethanol (C₂H₅OH). Understand stoichiometric calculations and mole ratios using a balanced equation. Suitable for students in Grades 10-12.

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