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Reaction I. Cu(s) + ? Cu(NO3)2 (aq) + NO2 (g) Reaction II. Cu(NO3)2 (aq) + ? Cu(OH) Reaction III. Cu(OH)2 (s) + ? CuO (s) + H Reaction IV. CuO (s) +

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Reaction I. Cu(s) + ? → Cu(NO3)2 (aq) + NO2 (g) Reaction II. Cu(NO3)2 (aq) + ? → Cu(OH) Reaction III. Cu(OH)2 (s) + ? → CuO (s) + H Reaction IV. CuO (s) + ? → CuSO Reaction V. CuSO4 (aq) + ? → Cu (s) For each step of the cycle, classify and write a balanced chemical equation for the reaction. a. If the reaction is an oxidation-reduction reaction: i. Write the half-reactions and label as oxidation or reduction. ii. Balance each half-reaction. iii. Balance the electrons. iv. Summarized the half-reactions to obtain a balanced chemical equation for the reaction. b. If the reaction is a precipitation or acid/base reaction, write the formula unit equation, the total ionic and net ionic equations. c. If the reaction is decomposition reaction, write a balanced chemical equation
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electrons are already balanced. cant u see... View the full answer

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