**Passage 9:** moles of is decomposed completely. The gas evolved is used to oxidize to . <br> **Q1: — Redox Reactions and Volumetric Analysis Chemistry Question
Question
**Passage 9:** $0.2$ moles of $KClO_3$ is decomposed completely. The $O_2$ gas evolved is used to oxidize $H_2S$ to $S$. <br> **Q1:** The volume of $O_2$ evolved at STP is:
Answer: A
💡 Solution & Explanation
**Step 1:** $2KClO_3 \rightarrow 2KCl + 3O_2$. <br>**Step 2:** $2$ moles $KClO_3$ gives $3$ moles $O_2$. <br>**Step 3:** $0.2$ moles $KClO_3$ gives $0.3$ moles $O_2$. <br>**Step 4:** Vol = $0.3 \times 22.4 = 6.72$ L.
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