We’re being asked to calculate for the mass of potassium chlorate (KClO3) that decomposes into potassium chloride (KCl) and 638 mL of O2.
Decomposition reaction: 2 KClO3(s) ⟶2 KCl(s) + 3 O2(g)
We’re going to calculate the mass of potassium chlorate using the following steps.
Step 1. Calculate the moles of O2 produced using the ideal gas equation.
P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K
Step 2. Calculate the moles of KClO3 decomposed using mol to mol comparison.
Step 3. Calculate the mass of KClO3 decomposed using its molar mass.
How many grams of potassium chlorate decompose to potassium chloride and 638 mL of O2 at 128°C and 752 torr?
2 KClO3(s) ⟶2 KCl(s) + 3 O2(g)
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Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
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Based on our data, we think this problem is relevant for Professor Donovan's class at UAKRON.
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.