Question

Given the equations A, B, C, and D:

(A) AgNO3 + NaCl → AgCl + NaNO3
(B) Cl2 + H2O → HClO + HCl
(C) CuO + CO → CO2 + Cu
(D) NaOH + HCl → NaCl + H2O


Which two equations represent redox reactions?

Answer 1

B and C

Step-by-step explanation:

(A) AgNO₃ + NaCl → AgCl + NaNO₃

This is a double displacement reaction. It is not a redox reaction because the elements have the same oxidation numbers on both sides.

(B) Cl₂ + H₂O → HClO + HCl

This is a redox reaction.

Cl₂ is oxidized to HClO. The oxidation number of Cl increases from 0 to +1.

Cl₂ is reduced to HCl. The oxidation number of Cl decreases from 0 to -1.

(C) CuO + CO → CO₂ + Cu

This is a redox reaction.

CO is oxidized to CO₂. The oxidation number of C increases from +2 to +4.

CuO is reduced to Cu. The oxidation number of Cu decreases from +2 to 0.

(D) NaOH + HCl → NaCl + H₂O

This is a double displacement reaction. It is not a redox reaction because the elements have the same oxidation numbers on both sides.