Balance the 1/2 reaction using the 1/2 rxn method: MnO_4^- (aq) rightarrow MrvO_2(aq) (basic) Skip 4d...
Balance the following redox reactions under both acidic and basic conditions I_2O_5(s) + CO(g) rightarrow I_2(s) + CO_2 (g) IO^- _3 + H_3AsO_3(aq) rightarrow H_3AsO_4(aq) + I_2(s) PbSO_4(s) + Br_2(I) rightarrow Pb(s) +SO^-2 _4(aq) +BrO^- _3(aq)
When the reaction MnO_4^-(aq) + CN^-(aq) rightarrow MnO_2(s) + CNO^-(aq) is balanced in a basic medium, what are the sum of the coefficients. 20 10 8 13 11
A method for determining the quantity of dissolved of oxygen in natural waters requires a series of redox reaction. Balance the following chemical equations in that series under the conditions indicated: a. In basic solution; Mn^2+(aq) + O_2(g) rightarrow MaO_2(g) b. In acidic solution; Mn^+2 O_2(s) + 2I^- rightarrow Mn^2+(aq) + I_2(s) c. In neutral solution; I_2(s) + S_2 O_3^2-(aq) rightarrow2I^-(a) + S_4O_6^2-(aq)
Balance the following reaction, using the half-reaction method, in basic solution. Cr^3+ (aq) + CIO (aq) rightarrow CI_2(aq) + CrO_4^2- (aq)
More Practice Balancing Redox Reactions in Acid and Basic Solution Balance the following redox reaction in both acidic and basic solution using the half reaction method outlined in Recitation 10, Part III. 3. Unbalanced: PbO2(s) + Mn2+(aq) → Pb2+ (aq) + MnO4- (aq) 4. Unbalanced: SO42-(aq) + Cr3+(aq) → SO2(g) + Cr2O72-(aq)
Balance the reaction in acidic conditions Pbo_2(8) + I^-(aq) rightarrow Pb^2+(aq) + I_2(s) I_2(s) rightarrow I^-(aq)
47 3. Balance the following redox reaction under acidic conditions using the half-reaction method. Na2S2O3 (aq) + 12 (aq) → Nal (aq) + Na2S406 (aq)
1. (3 points) Balance the following redox reaction under acidic aqueous conditions using the smallest whole-number coefficients possible. Mnog(aq) + HSQ (aq) → Mn(aq) + SO (aq) 2. (3 Points) Balance the following redox reaction under acidic aqueous conditions using the smallest whole-number coefficients possible. Croc-(aq) + C12(aq) → OC1-(aq) + Craq)
Find the emf of the cell described by the cell diagram Fe | Fe^2+ (1.500M) || Au^3+ (0.00400M) | Au. A) 1.99 V B) 1.89 V C) 1.94 V D) 1.66 V E) 1.91 V Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell? A) Zn^2+ (aq) + Ca(s) rightarrow Zn(s) + Ca^2+ (aq) B) Al^3+ (aq) + 3Br^- (aq) rightarrow Al(s) + (3/2)Br_2 (1) C) 2Al(s) + 3Fe^2+...
Use the half-reaction method to balance the following equation in basic solution: CN^- + MnO_4^- Right arrow CNO^- + MnO_2