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Standard XII

Chemistry

Kinetic Theory of Gases

Calculate the...

Question

Calculate the moles of $S O_{2}$ produced by burning $1.0$ metric ton $(10^{3} k g)$ of coal containing $0.05 %$ by mass of pyrites impurity.

8.32

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4.16

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12.48

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2.08

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Solution

The correct option is A $8.32$
The mass of $F e S_{2}$ present in 1000 kg of coal is $10^{6} \times \frac{0.05}{100} = 500$ g.
The molar mass of $F e S_{2}$ is 120.
The number of moles of $F e S_{2}$ in 500 g are $\frac{500}{120} = 4.17$ moles.
2 moles of $F e S_{2}$ will produce 4 moles of $S O_{2}$ .
1 mole of $F e S_{2}$ will produce 2 moles of $S O_{2}$ .
4.17 moles of $F e S_{2}$ will produce $2 \times 4.17 = 8.32$ moles of $S O_{2}$ .

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Calculate the moles of SO2 produced by burning 1.0 metric ton (103 kg) of coal containing 0.05% by mass of pyrites impurity.

Calculate the moles of $S O_{2}$ produced by burning $1.0$ metric ton $(10^{3} k g)$ of coal containing $0.05 %$ by mass of pyrites impurity.