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 = 20.61 g Mass crucible + lid+ KClO3/KCl mixture = 26.11 g
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 = 20.61 g
Mass crucible + lid+ KClO3/KCl mixture = 26.11 g
After Heating
Mass crucible + lid+ contents (after final heating ) = 24.68 g
a) Mass KClO3 in mixture (stoichiometric calculation from the mass of oxygen evolved)
b) %KClO3 in mixture (g KClO3/g mixture then multiply by 100)
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