QuestionMay 24, 2025

Do this problem on your own. Starting with 9.2 moles of O_(2) how many moles of H_(2)S will you need, and how many moles of SO_(2) will you get? (you should have TWO answers 6.2mol H_(2)S and 6.2molSO_(2) 6.2mol H_(2)S and 9.2mol SO_(2) 9.2mol H_(2)S and 9.2mol SO_(2)

Do this problem on your own. Starting with 9.2 moles of O_(2) how many moles of H_(2)S will you need, and how many moles of SO_(2) will you get? (you should have TWO answers 6.2mol H_(2)S and 6.2molSO_(2) 6.2mol H_(2)S and 9.2mol SO_(2) 9.2mol H_(2)S and 9.2mol SO_(2)
Do this problem on your own. Starting with 9.2 moles of O_(2) how many moles of H_(2)S will you need, and how many moles of SO_(2) will you get? (you should have TWO answers 6.2mol H_(2)S and 6.2molSO_(2) 6.2mol H_(2)S and 9.2mol SO_(2) 9.2mol H_(2)S and 9.2mol SO_(2)

Solution
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Answer

6.13 mol H_2S and 6.13 mol SO_2 Explanation 1. Write the balanced chemical equation The reaction is 2H_2S + 3O_2 \rightarrow 2SO_2 + 2H_2O. 2. Determine mole ratio from the equation From the balanced equation, the mole ratio of O_2 to H_2S is 3:2, and O_2 to SO_2 is 3:2. 3. Calculate moles of H_2S needed Using the ratio 3:2, for 9.2 moles of O_2, moles of H_2S needed = \frac{2}{3} \times 9.2 = 6.13 moles. 4. Calculate moles of SO_2 produced Using the same ratio 3:2, moles of SO_2 produced = \frac{2}{3} \times 9.2 = 6.13 moles.

Explanation

1. Write the balanced chemical equation<br /> The reaction is $2H_2S + 3O_2 \rightarrow 2SO_2 + 2H_2O$.<br /><br />2. Determine mole ratio from the equation<br /> From the balanced equation, the mole ratio of $O_2$ to $H_2S$ is 3:2, and $O_2$ to $SO_2$ is 3:2.<br /><br />3. Calculate moles of $H_2S$ needed<br /> Using the ratio 3:2, for 9.2 moles of $O_2$, moles of $H_2S$ needed = $\frac{2}{3} \times 9.2 = 6.13$ moles.<br /><br />4. Calculate moles of $SO_2$ produced<br /> Using the same ratio 3:2, moles of $SO_2$ produced = $\frac{2}{3} \times 9.2 = 6.13$ moles.
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