According to the following balanced reaction,how many moles of KO are required to exactly react with 4.33 moles of H₂O?
4 KO(s) + 2 H₂O(l) → 4 KOH(s) + O₂(g)

Question

According to the following balanced reaction,how many moles of KO are required to exactly react with 4.33 moles of H₂O? 4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

Quizplus · Accepted Answer

According to the balanced chemical equation, 4 moles of KO reacts with 2 moles of H₂O. Therefore, 1 mole of KO reacts with 0.5 moles of H₂O. To react with 4.33 moles of H₂O, we need: 4.33 mol H₂O × 1 mol KO/0.5 mol H₂O = 8.66 mol KO Therefore, the answer is B.

According to the Following Balanced Reaction,how Many Moles of KO