Sure, let's break it down step-by-step based on the balanced chemical equation:
[tex]\[
8 H_2 + S_8 \rightarrow 8 H_2S
\][/tex]
The balanced equation tells us the molar ratios in which the reactants combine to form the products. Specifically:
1. Mole Ratios:
- For every 8 moles of [tex]\(H_2\)[/tex] (hydrogen), there is 1 mole of [tex]\(S_8\)[/tex] (sulfur).
- This reaction produces 8 moles of [tex]\(H_2S\)[/tex] (hydrogen sulfide).
2. Predictions Based on Mole Ratios:
- If we have 1 mole of [tex]\(H_2\)[/tex], how much [tex]\(S_8\)[/tex] will react with it?
- According to the balanced equation, 8 moles of [tex]\(H_2\)[/tex] react with 1 mole of [tex]\(S_8\)[/tex]. This simplifies to the ratio of [tex]\(8:1\)[/tex].
- So, 1 mole of [tex]\(H_2\)[/tex] would require [tex]\(\frac{1}{8}\)[/tex] mole of [tex]\(S_8\)[/tex] for the reaction.
- Therefore, the statement "1 mol of hydrogen will react with 1 mol of sulfur" is incorrect.
3. Cross-verify Other Options:
- [tex]\(8 \text{ mol of hydrogen will react with 1 mol of sulfur}\)[/tex]:
- This statement matches perfectly with the given balanced equation. For every 8 moles of [tex]\(H_2\)[/tex], 1 mole of [tex]\(S_8\)[/tex] is used. This statement is correct.
- [tex]\(8 \text{ mol of hydrogen will react with 8 mol of sulfur}\)[/tex]:
- This suggests an [tex]\(8:8\)[/tex] ratio, which contradicts the balanced equation.
- [tex]\(16 \text{ mol of hydrogen will react with 8 mol of sulfur}\)[/tex]:
- This suggests a [tex]\(16:8\)[/tex] ratio, which also contradicts the balanced equation ratio of [tex]\(8:1\)[/tex].
Based on these considerations, the most likely prediction from the balanced equation [tex]\(8 H_2 + S_8 \rightarrow 8 H_2S\)[/tex] is that:
8 mol of hydrogen will react with 1 mol of sulfur.
