Questions: 2 KClO3 -> 2 KCl + 3 O2 How many moles of O2 will be formed from 1.65 moles of KClO2 ? (0.25 pt / ea space) 1.65 mol KClO3 -mol O2 -mol KClO3 = mol OO2

Transcript text: \[ 2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl}+3 \mathrm{O}_{2} \] How many moles of $\mathrm{O}_{2}$ will be formed from 1.65 moles of $\mathrm{KClO}_{2}$ ? $(0.25 \mathrm{pt} / \mathrm{ea}$ space $)$ $\left.$\begin{tabular}{c|c|} $1.65 \mathrm{~mol} \mathrm{KClO}_{3}$ & $-\mathrm{mol} \mathrm{O}_{2}$ \\ \hline & $-\mathrm{mol} \mathrm{KClO}_{3}$ \end{tabular} \right\rvert\,$=$ $\qquad$ $\mathrm{mol} \mathrm{O} \mathrm{O}_{2}$

Solution

Solution Steps

Step 1: Understand the Chemical Reaction

The balanced chemical equation is:

\[ 2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl} + 3 \mathrm{O}_{2} \]

This equation tells us that 2 moles of $\mathrm{KClO}_{3}$ decompose to produce 3 moles of $\mathrm{O}_{2}$.

Step 2: Set Up the Mole Ratio

From the balanced equation, the mole ratio of $\mathrm{KClO}_{3}$ to $\mathrm{O}_{2}$ is 2:3. This means for every 2 moles of $\mathrm{KClO}_{3}$, 3 moles of $\mathrm{O}_{2}$ are produced.

Step 3: Calculate Moles of $\mathrm{O}_{2}$

Given 1.65 moles of $\mathrm{KClO}_{3}$, we can use the mole ratio to find the moles of $\mathrm{O}_{2}$:

\[ \text{Moles of } \mathrm{O}_{2} = 1.65 \, \text{moles of } \mathrm{KClO}_{3} \times \frac{3 \, \text{moles of } \mathrm{O}_{2}}{2 \, \text{moles of } \mathrm{KClO}_{3}} \]

\[ = 1.65 \times \frac{3}{2} = 2.475 \, \text{moles of } \mathrm{O}_{2} \]