How would you balance the following equation: S+HNO3 --> H2SO4+NO2+H2O?

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How would you balance the following equation: S+HNO3 --> H2SO4+NO2+H2O?

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Answer 1 · 2016-01-27T20:15:40

By a redox reaction. Sulfur is oxidized to sulfate; nitrate is reduced to nitric oxide:

$S (s) + 6 N O_{3}^{-} + 4 H^{+} \to 6 N O_{2} (g) ↑ ⏐ ⏐ + 2 H_{2} O (l) + S O_{4}^{2 -}$ $S(s) + 6NO_3^(-) + 4H^+ rarr 6NO_2(g)uarr + 2H_2O(l) + SO_4^(2-)$

Explanation:

Reduction:
$N O_{3}^{-} + 2 H^{+} + e^{-} \to N O_{2} (g) ↑ ⏐ ⏐ + H_{2} O$ $NO_3^(-) + 2H^(+) +e^(-) rarr NO_2(g)uarr + H_2O$ $(i)$ $(i)$

Oxidation:
$S (s) + 4 H_{2} O (l) \to S O_{4}^{2 -} + 8 H^{+} + 6 e^{-}$ $S(s) + 4H_2O(l) rarr SO_4^(2-) + 8H^+ + 6e^-$ $(i i)$ $(ii)$

$(i i) + 6 \times (i)$ $(ii) + 6xx(i)$ $=$ $=$ $S (s) + 4 H N O_{3} (a q) + 2 N O_{3}^{-} \to 6 N O_{2} (g) ↑ ⏐ ⏐ + 2 H_{2} O (l) + S O_{4}^{2 -}$ $S(s) + 4HNO_3(aq) + 2NO_3^(-) rarr 6NO_2(g)uarr + 2H_2O(l) + SO_4^(2-)$

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How would you balance the following equation: S+HNO3 --> H2SO4+NO2+H2O?

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