Consider the following unbalanced equation:
KO₂ + H₂O → KOH + O₂ + H₂O₂
For every 3.0 mol of KO₂, ___ mol of H₂O is needed for a complete reaction.

Question

Consider the following unbalanced equation: KO₂ + H₂O → KOH + O₂ + H₂O₂ For every 3.0 mol of KO₂, ___ mol of H₂O is needed for a complete reaction.

Quizplus · Accepted Answer

The balanced equation is: 2KO₂ + 2H₂O → 2KOH + O₂ + H₂O₂ Therefore, for every 2 mol of KO₂, 2 mol of H₂O is needed. To find how much H₂O is needed for 3.0 mol of KO₂, we can set up a proportion: 2 mol KO₂ / 2 mol H₂O = 3.0 mol KO₂ / x mol H₂O Simplifying the proportion gives: x = (2 mol H₂O * 3.0 mol KO₂) / 2 mol KO₂ = 3.0 mol H₂O Therefore, the answer is C) 3.0.

Consider the Following Unbalanced Equation