According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 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 5.44 moles of H₂O? 4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

Quizplus · Accepted Answer

According to the balanced reaction, 4 moles of KO react with 2 moles of H₂O. This means that to completely react with 1 mole of H₂O, we need 4/2 = 2 moles of KO. Therefore, to exactly react with 5.44 moles of H₂O, we will need 5.44 x 2 = 10.88 moles of KO. Rounded to the nearest tenth, this is 10.9 moles of KO, which is answer choice B.

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