Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction

Identify the following reactions as acid-base, precipitation, or redox reactions. 5 Ca(OH)2(aq) + 3PO4(aq) → Ca5OH(PO4)3(s) + 9 OH(aq) Give detailed Solution of all reactions. don't give Handwritten answer. Ca(OH)2(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + 2 H2O(aq) precipitation precipitation 8 H+(aq) + MnO4(aq) + Fe2+(aq) → Mn2+(aq) + Fe3+(aq) + 4 H2O() precipitation 12(s) + 2 S2032(aq) → S4062(aq) + 2(aq) redox

Complete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. CrO42–(aq) + Cu (s) → Cr(OH)3 (s) + Cu(OH)2 (s)     In the balanced equation, 3 molecules of water are present on the product side.     In the balanced equation, 3 molecules of water are present on the reagent side.     In the balanced equation, 4 OH- are present on the reagent side.     In the balanced equation, 4 OH- are present on the product side.     In the balanced equation, 5 molecules of water are present on the product side.     In the balanced equation, 5 molecules of water are present on the reagent side.

Balance the following redox reaction that occurs in acidic conditions: Pt(s) + NO₃⁻(aq) + Cl⁻(aq) ⟶ PtCl₆²⁻ (aq) + NO₂(g)