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The chemical equation provided is:

\[
2H_2(g) + O_2(g) \rightarrow 2H_2O(l)
\]

This represents the reaction between hydrogen gas (\(H_2\)) and oxygen gas (\(O_2\)) to form water (\(H_2O\)).

From the balanced equation, you can see that:
- 2 moles of \(H_2\) react with 1 mole of \(O_2\) to form 2 moles of \(H_2O\).

The question asks how many moles of oxygen gas (\(O_2\)) are needed to form **1 mole** of water (\(H_2O\)).

Since the equation shows that 1 mole of oxygen gas reacts to form 2 moles of water, to form **1 mole of water**, you would need **half a mole** of oxygen gas (\(O_2\)).

Thus, the answer is:
\[
0.5 \text{ moles of } O_2
\]

Would you like more details or have any questions?

Here are 5 related questions:
1. What is the mole ratio between \(H_2\) and \(O_2\) in the reaction?
2. How many moles of \(H_2\) are needed to produce 4 moles of water?
3. If you have 2 moles of oxygen, how many moles of water can you form?
4. What is the mass of oxygen gas required to form 1 mole of water?
5. How many moles of water would be produced from 3 moles of \(O_2\)?

**Tip:** Always balance a chemical equation before performing stoichiometric calculations to ensure that the mole ratios are accurate.

Consider the chemical equation shown below: How many moles of oxygen gas are needed to react with hydrogen to form one mole of water?

Learn how to determine the number of moles of oxygen gas needed to produce one mole of water using stoichiometry and balanced chemical equations.

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