When water was electrolyzed, hydrogen and oxygen were obtained which were collected and found to be $16.8$ L at $S T P$ . Then, weight of water electrolyzed is:

18

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36

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9

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45

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Solution

The correct option is C $9$ gm
The balanced chemical equation for the electrolysis of water is $2 H_{2} O \to 2 H_{2} + O_{2}$ .
Thus, $2$ moles of water $(2 \times 18 = 36 g)$ on electrolysis gives $3$ moles $(3 \times 22.4 L)$ of hydrogen and oxygen at STP together.
Hence, $16.8$ L of hydrogen and oxygen at STP corresponds to $\frac{36 g}{3 \times 22.4 L} \times 16.8 L = 9 g$ .
Hence, the weight of water electrolyzed is $9$ g.

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When water was electrolyzed, hydrogen and oxygen were obtained which were collected and found to be 16.8 L at STP. Then, weight of water electrolyzed is:

When water was electrolyzed, hydrogen and oxygen were obtained which were collected and found to be $16.8$ L at $S T P$ . Then, weight of water electrolyzed is: