Which of the following reactions are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those reactions that are not redox reactions, indicate whether they are precipitation or neutralization reactions.
a. P4 (s) + 10 HClO (aq) + 6 H2O (l) → 4 H3PO4 (aq) + 10 HCl (aq)
b. Br2 (l) + 2 K (s) → 2 KBr (s)
c. CH3CH2OH (l) + 3 O2 (g) → 3 H2O (l) + CO2 (g)
d. ZnCl2 (aq) + 2 NaOH (aq) → Zn(OH)2 (s) + 2 NaCl (aq)
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a. This is a redox reaction. Phosphorus (P) is oxidized from an oxidation state of 0 to an oxidation state of +5 in H3PO4 (aq). Chlorine (Cl) is reduced from an oxidation state of +1 to an oxidation state of -1 in HCl (aq).
b. This is not a redox reaction. It is a combination reaction where two elements, Br2 (l) and K (s), combine to form a compound, KBr (s).
c. This is a redox reaction. Carbon (C) is oxidized from an oxidation state of -2 in CH3CH2OH (l) to an oxidation state of +4 in CO2 (g). Oxygen (O) is reduced from an oxidation state of 0 in O2 (g) to an oxidation state of -2 in H2O (l).
d. This is not a redox reaction. It is a double displacement reaction where ZnCl2 (aq) and NaOH (aq) switch partners to form Zn(OH)2 (s) and NaCl (aq).
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