$4.90$ g of $K C l O_{3}$ , on heating shows a weight loss of $0.384 g$ . What percentage of the original $K C l O_{3}$ has decomposed?

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Solution

$2 K C l O_{3} + h e a t \to 2 K C l + 3 O_{2}$
2mol $K C l O_{3}$ produce 3 mol $O_{2}$
The 0.384 g mass loss was due to the oxygen generated.
The amount of moles of oxygen generated can be calculated as: Molar mass $O_{2}$ = 32 g/mol
0.384 g $O_{2}$ = 0.384/32 = 0.012 mol $O_{2}$ generated
This came from the decomposition of 0.012 x 2/3 = 0.008 mol of $K C l O_{3}$
Molar mass $K C l O_{3}$ = 122.55 g/mol
0.008 mol $K C l O_{3}$ = 0.008 x 122.55 = 0.9804 g $K C l O_{3}$ decomposed
% of original sample $= \frac{0.9804}{4.90} \times 100 = 20 %$

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