Problem: A mixture of KClO3 and KCl with a mass of 0.950 g was heated to produce O2. After heating, the mass of residue was 0.700 g. Assuming all the KClO3 decomposed to KCl and O2, calculate the mass percent of KClO3 in the original mixture.

🤓 Based on our data, we think this question is relevant for Professor Foster's class at GMU.

FREE Expert Solution

We are asked to calculate the mass percent of KClO3 in the original mixture. 


Step 1. Calculate mass O2 produced 

2  KClO3 → 2 KCl + 3 O2 

KCl → residue


Mass Mixture = Mass KClO3 + Mass KCl 

Mass Mixture = (Mass KCl + Mass O2) + Mass KCl

Mass Mixture = (Mass KCl + Mass KCl) + Mass O2

Mass Mixture = (Mass Residue) + Mass O2

Mass O2 = Mass Mixture - Mass Residue

Mass O2 = 0.950 g - 0.700 g

Mass O2 = 0.250 g


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Problem Details

A mixture of KClO3 and KCl with a mass of 0.950 g was heated to produce O2. After heating, the mass of residue was 0.700 g. Assuming all the KClO3 decomposed to KCl and O2, calculate the mass percent of KClO3 in the original mixture.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Foster's class at GMU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.