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Q.

In a textile industry, chlorine is used to bleach fabrics. Any of the toxic chlorine that remains after the bleaching process is destroyed by reacting it with a sodium thiosulphate solution. If $52.7 k g N a_{2} S_{2} O_{3}$ is consumed to remove the chlorine what is the mass of the sulphur product formed in kilograms. (round to nearest integer)
At wts : Na = 23, Cl = 35.5, S =32, O = 16, H = 1

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answer is 80.

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Detailed Solution

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$\underset{158}{N a_{2} S_{2} O_{3}} + 4 C l_{2} + 5 H_{2} O \to \underset{240}{2 N a H S O_{4}} + 8 H C l$
If $158 k g$ of $N a_{2} S_{2} O_{3}$ is consumed $240 k g$ of $N a H S O_{4}$ will be formed
If $52.7 k g$ of $N a_{2} S_{2} O_{3}$ is consumed the wt of product formed is $\frac{52.7 \times 240}{158} = 80.05 k g$
=80kg

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