Answer :
To analyze the given chemical equation:
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
We need to understand the stoichiometry of the reaction. This equation tells us that 2 moles of hydrogen gas ([tex]\(H_2\)[/tex]) react with 1 mole of oxygen gas ([tex]\(O_2\)[/tex]) to produce 2 moles of water ([tex]\(H_2O\)[/tex]).
Now, let's break down what would happen if 1 mole of [tex]\(H_2\)[/tex] is used in this reaction, step-by-step:
1. The given equation shows that 2 moles of [tex]\(H_2\)[/tex] react with 1 mole of [tex]\(O_2\)[/tex]. This can be represented by the ratio:
[tex]\[ \frac{2 \text{ moles } H_2}{1 \text{ mole } O_2} = \frac{1 \text{ mole } H_2}{0.5 \text{ mole } O_2} \][/tex]
2. If we use 1 mole of [tex]\(H_2\)[/tex], we need to adjust the amount of [tex]\(O_2\)[/tex] proportionally. According to the ratio derived above:
- For 1 mole of [tex]\(H_2\)[/tex], we need 0.5 moles of [tex]\(O_2\)[/tex].
3. We also need to determine the amount of [tex]\(H_2O\)[/tex] produced:
[tex]\[ 2 \text{ moles } H_2 \rightarrow 2 \text{ moles } H_2O \][/tex]
Therefore, for 1 mole of [tex]\(H_2\)[/tex], using the same stoichiometric relationship:
- 1 mole of [tex]\(H_2\)[/tex] will produce 1 mole of [tex]\(H_2O\)[/tex].
Now, let's examine the given statements based on our analysis:
- "One mole of oxygen was used in this reaction."
This statement is incorrect. Only 0.5 moles of [tex]\(O_2\)[/tex] are needed for 1 mole of [tex]\(H_2\)[/tex].
- "Two moles of oxygen were used in this reaction."
This statement is incorrect. It's even further from our calculated 0.5 moles of [tex]\(O_2\)[/tex].
- "One mole of water was produced from this reaction."
This statement is correct. 1 mole of [tex]\(H_2\)[/tex] produces 1 mole of [tex]\(H_2O\)[/tex].
- "Two moles of water were produced from this reaction."
This statement is incorrect. Only 1 mole of [tex]\(H_2O\)[/tex] is produced from 1 mole of [tex]\(H_2\)[/tex].
Therefore, the correct statement is:
- One mole of water was produced from this reaction.
[tex]\[ 2 H_2 + O_2 \rightarrow 2 H_2O \][/tex]
We need to understand the stoichiometry of the reaction. This equation tells us that 2 moles of hydrogen gas ([tex]\(H_2\)[/tex]) react with 1 mole of oxygen gas ([tex]\(O_2\)[/tex]) to produce 2 moles of water ([tex]\(H_2O\)[/tex]).
Now, let's break down what would happen if 1 mole of [tex]\(H_2\)[/tex] is used in this reaction, step-by-step:
1. The given equation shows that 2 moles of [tex]\(H_2\)[/tex] react with 1 mole of [tex]\(O_2\)[/tex]. This can be represented by the ratio:
[tex]\[ \frac{2 \text{ moles } H_2}{1 \text{ mole } O_2} = \frac{1 \text{ mole } H_2}{0.5 \text{ mole } O_2} \][/tex]
2. If we use 1 mole of [tex]\(H_2\)[/tex], we need to adjust the amount of [tex]\(O_2\)[/tex] proportionally. According to the ratio derived above:
- For 1 mole of [tex]\(H_2\)[/tex], we need 0.5 moles of [tex]\(O_2\)[/tex].
3. We also need to determine the amount of [tex]\(H_2O\)[/tex] produced:
[tex]\[ 2 \text{ moles } H_2 \rightarrow 2 \text{ moles } H_2O \][/tex]
Therefore, for 1 mole of [tex]\(H_2\)[/tex], using the same stoichiometric relationship:
- 1 mole of [tex]\(H_2\)[/tex] will produce 1 mole of [tex]\(H_2O\)[/tex].
Now, let's examine the given statements based on our analysis:
- "One mole of oxygen was used in this reaction."
This statement is incorrect. Only 0.5 moles of [tex]\(O_2\)[/tex] are needed for 1 mole of [tex]\(H_2\)[/tex].
- "Two moles of oxygen were used in this reaction."
This statement is incorrect. It's even further from our calculated 0.5 moles of [tex]\(O_2\)[/tex].
- "One mole of water was produced from this reaction."
This statement is correct. 1 mole of [tex]\(H_2\)[/tex] produces 1 mole of [tex]\(H_2O\)[/tex].
- "Two moles of water were produced from this reaction."
This statement is incorrect. Only 1 mole of [tex]\(H_2O\)[/tex] is produced from 1 mole of [tex]\(H_2\)[/tex].
Therefore, the correct statement is:
- One mole of water was produced from this reaction.
