Dvide the following redox equations into oxidation half equation and reduction half equation.
$a) P_{(s)} + P O_{4 (a q)}^{3} H P O_{3 (a q)}^{2} b) H N O_{2 (a q)} ⟶ N O_{3 (a q)}^{-} + N O_{(g)} c) I O_{3 (a q)}^{-} + {R e}_{(s)} ⟶ R e O_{4 (a q)} + I_{(a q)}$

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Solution

(a) $0 P (s) + + 5 P O_{4}^{3 -} (a q) \to + 3 H P O_{3}^{2 -} (a q)$
Oxidation :- $0 P (s) \to + 3 H P O_{3}^{2 -} (a q)$
Reduction : $+ 5 P O_{4}^{3 -} (a q) \to + 3 H P O_{3}^{2 -} (a q)$
(b) $+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-} (a q) + + 2 N O (g)$
Oxidation :- $+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-} (a q)$
Reduction : $+ 3 H N O_{2} (a q) \to + 2 N O_{2} (g)$
(c) $+ 7 I O_{3}^{-} (a q) + 0 R e (s) \to + 8 R e O_{4} (a q) + 0 I (a q)$
Oxidation : $0 R e (s) \to + 8 R e O_{4} (a q)$
Reduction : $+ 7 I O_{3}^{-} (a q) \to 0 I (a q)$

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