1st find mol of O2
Given:
P = 1.0 atm
V = 143.0 mL
= (143.0/1000) L
= 0.143 L
T = 273.0 K
find number of moles using:
P * V = n*R*T
1 atm * 0.143 L = n * 0.08206 atm.L/mol.K * 273 K
n = 6.383*10^-3 mol
From reaction,
Mol of KClO reacted = (2/3)* mol of O2 formed
= (2/3)*6.383*10^-3 mol
= 4.26*10^-3 mol
Molar mass of KClO,
MM = 1*MM(K) + 1*MM(Cl) + 1*MM(O)
= 1*39.1 + 1*35.45 + 1*16.0
= 90.55 g/mol
use:
mass of KClO,
m = number of mol * molar mass
= 4.26*10^-3 mol * 90.55 g/mol
= 0.3857 g
Now use:
Mass % of KClO = mass of KClO * 100 / mass of mixture
= 0.3857 * 100 / 1.34
= 28.8 %
Answer: 28.8 %
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A mixture contains KClO3 and KCl. When the mixture is heated, only the KClO3 decomposes via the following reaction: 2KClO3 (s) → 3O2 (g) + 2KCl (s) In an experiment to determine the percent KClO3 in a KClO3/KCl mixture, the mixture was heated in a crucible several times in order to bring it to constant mass. The following experimental data was obtained. Before Heating Mass empty crucible + lid = 21.77 g Mass crucible + lid+ KClO3/KCl mixture = 26.16...
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