The amount of water produced (in $g$ ) in the oxidation of 1 mole of rhombic sulphur by conc. $H N O_{3}$ to a compound with the highest oxidation state of sulphur is
(Given data: Molar mass of water = 18 $g m o l^{- 1}$ )

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Solution

The corresponding reaction of rhombic sulphur and conc. $H N O_{3}$ is
$S_{8} + 48 H N O_{3} \to 8 H_{2} S O_{4} + 48 N O_{2} + 16 H_{2} O$

Mass of $H_{2} O = 18 \times 16 = 288 g$

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The highest stable oxidation state exhibited by sulphur in its compounds is:

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H_{2} S O_{4}

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H_{2} S O_{4}

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