Let's analyze the given chemical equation:
[tex]\[
2 H_2 + O_2 \rightarrow 2 H_2 O
\][/tex]
This equation tells us the stoichiometric ratios of the reactants and products. Specifically:
- 2 moles of hydrogen gas (\(H_2\)) react with 1 mole of oxygen gas (\(O_2\)) to produce 2 moles of water (\(H_2O\)).
Now let's see what happens when one mole of \(H_2\) is used in this reaction.
1. Reactants:
According to the equation, 2 moles of \(H_2\) react with 1 mole of \(O_2\).
- Therefore, if we use 1 mole of \(H_2\), we need \( \frac{1}{2} \) mole of \(O_2\) to react with it. This means 0.5 moles of \(O_2\) is required.
2. Products:
The equation also tells us that 2 moles of \(H_2\) produce 2 moles of \(H_2O\).
- Therefore, using 1 mole of \(H_2\) would produce exactly 1 mole of \(H_2O\).
Let's match the findings with the given statements:
1. One mole of oxygen was used in this reaction. (Incorrect: 0.5 moles of \(O_2\) was used.)
2. Two moles of oxygen were used in this reaction. (Incorrect: 0.5 moles of \(O_2\) was used.)
3. One mole of water was produced from this reaction. (Correct: 1 mole of \(H_2O\) was produced.)
4. Two moles of water were produced from this reaction. (Incorrect: 1 mole of \(H_2O\) was produced.)
Therefore, the correct statement is:
One mole of water was produced from this reaction.
