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Question

$$4.90$$ g of $$KClO_3$$, on heating shows a weight loss of $$0.384g$$. What percentage of the original $$KClO_3$$ has decomposed?


Solution

$$2KClO_{3} + heat \rightarrow  2KCl + 3O_{2}$$
2mol $$KClO_{3}$$ 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$$KClO_3$$
Molar mass $$KClO_3$$  = 122.55 g/mol 
0.008 mol $$KClO_3$$ = 0.008 x 122.55 = 0.9804 g $$KClO_3$$ decomposed
% of original sample$$=\dfrac{0.9804}{4.90}\times 100=20\%$$

Chemistry

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