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Standard XII

Chemistry

Percentage Composition

In a small-sc...

Question

In a small-scale experiment, 10 g of $K C l O_{3}$ was carefully decomposed and 3.41 g of $O_{2}$ gas was collected. What are the theoretical(g), actual(g) and percent (%) yields of the reaction?

3.41 g, 3.92 g, 87%

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5.57 g, 6.12 g, 68 %

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3.92 g, 3.41 g, 87 %

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6.59 g, 3.41 g, 34 %

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Solution

The correct option is C 3.92 g, 3.41 g, 87 %
Reaction: $2 K C l O_{3} \to 2 K C l + 30_{2}$
Molar mass of $K C l O_{3} = 122.5$ g/mole
According to the reaction,
2 moles of $K C l O_{3}$ decomposes to 3 moles of $O_{2}$
$(2 \times$ 122.5 g) $K C l O_{3}$ decomposes to $3 \times$ 32 g of $O_{2}$
So, 10 g of $K C l O_{3}$ will produce $\frac{3 \times 32}{2 \times 122.5} \times 10 = 3.92$ g
Theoretical yield = 3.92 g; Actual yield = 3.41g
% yield $= \frac{actual yield}{theoretical yield} \times 100 = \frac{3.41}{3.92} \times 100 = 87$ %

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Percentage Composition

Standard XII Chemistry

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In a small-scale experiment, 10 g of KClO3 was carefully decomposed and 3.41 g of O2 gas was collected. What are the theoretical(g), actual(g) and percent (%) yields of the reaction?

In a small-scale experiment, 10 g of $K C l O_{3}$ was carefully decomposed and 3.41 g of $O_{2}$ gas was collected. What are the theoretical(g), actual(g) and percent (%) yields of the reaction?