Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Crand Cl₂ in the balanced reaction? Cr(s)+ Cl₂(g)→ Cr³⁺(aq)+ Cl^-(aq) A) Cr = 2, Cl₂ = 3 B) Cr = 2, Cl₂ = 4 C) Cr = 1, Cl₂ = 2 D) Cr = 2, Cl₂ = 1 E) Cr = 3, Cl₂ = 2

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In a basic solution, the half-reaction for the oxidation of Cr is:Cr(s) → Cr(OH)3(aq) + 3e-The half-reaction for the reduction of Cl2 is:Cl2(g) + 2e- → 2Cl-(aq)To balance the number of electrons lost and gained, we multiply the first half-reaction by 2 and the second half-reaction by 3:2Cr(s) → 2Cr(OH)3(aq) + 6e-3Cl2(g) + 6e- → 6Cl-(aq)Adding the two half-reactions, we get the overall balanced reaction:2Cr(s) + 3Cl2(g) → 2Cr(OH)3(aq) + 6Cl-(aq)

Balance the Following Redox Reaction If It Occurs in Basic