Question

Consider the following balanced equation:

2KCIO3(s) → 2KCl(s) + 302(g)
How many moles of O2 will be obtained by decomposing
3.50 moles of KCIO3?
0.530 mole
O 3.00 moles
O 2.30 moles
5.25 moles

Answer 1

5.25 moles

General Formulas and Concepts:

Chemistry

Atomic Structure

• Compounds
• Moles

Aqueous Solutions

• States of matter

Stoichiometry

• Analyzing reactions RxN
• Using Dimensional Analysis

Step-by-step explanation:

Step 1: Define

[RxN - Balanced] 2KClO₃ (s) → 2KCl (s) + 3O₂ (g)

[Given] 3.50 mol KClO₃

[Solve] mol O₂

Step 2: Identify Conversions

[RxN] 2 mol KClO₃ (s) → 3 mol O₂ (g)

Step 3: Stoichiometry

1. [DA] Set up conversion:
   `\displaystyle 3.50 \ mol \ KClO_3((3 \ mol \ O_2)/(2 \ mol \ KClO_3))`
2. [DA} Multiply [Cancel out units]:
   `\displaystyle 5.25 \ mol \ O_2`