Answered

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Read the chemical equation:

[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]

Which of the following statements would be correct if one mole of \( H_2 \) was used in this reaction?

A. One mole of oxygen was used in this reaction.
B. Two moles of oxygen were used in this reaction.
C. One mole of water was produced from this reaction.
D. Two moles of water were produced from this reaction.

Sagot :

GinnyAnswer
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.
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