Fc^2+ (aq) + Mo_3^- (aq) rightarrow Fe^3+ (aq) + No(g) acidic solution.
Balance the following redox equations: CrO_4^2- + Fe^2+ rightarrow Cr^3+ + Fe^3+ (in acidic solution) MnO^4^- + CIO_2^- rightarrow MnO^2 + CIO_4^- (in basic solution)
Balance the following in acidic conditions: I_2(l) + SO_2(g) rightarrow I^-(aq) + SO_4^2-(aq)
Calculate the standard cell potential for the following reaction. Fe (s) +Ni^+2 (aq) rightarrow Fe^+ 2 (aq) + Ni (s) 3 Cu + 2 NO_3^- + 8 H^+ rightarrow 3 Cu^+ 2+ 2 NO +4 H_2O Cr_2O_7^-2 + 6 Fe^+2+14 H6+ rightarrow 2 Cr^+ 3 + 6 Fe^+ 3 +7 H_2O
Balance the reaction
in acidic conditions
Pbo_2(8) + I^-(aq) rightarrow Pb^2+(aq) + I_2(s) I_2(s) rightarrow I^-(aq)
The E? values for two low-spin iron complexes in acidic solution are as follows: [Fe(o?phen)3]3+(aq)+e? ?[Fe(o?phen)3]2+(aq) E?=1.12V [Fe(CN)6]3?(aq)+e? ?[Fe(CN)6]4?(aq) E?=0.36V Part A Which complex is more difficult to reduce? [Fe(o-phen)3]3+ [Fe(CN)6]3? PArt B Is it thermodynamically favorable to reduce both Fe(III) complexes to their Fe(II) analogs? yes no
The following chemical reaction takes place in aqueous solution: Fe(NO_3)_2 (aq) + K_2S(aq) rightarrow FeS(s) + 2KNO_3(aq) Write the net ionic equation for this reaction.
Please include the physical state symbols
Balance the following redox reaction in acidic solution. Felt(ag)+NO, (ag) → Fc² (aq)+NO(g) Fe (aq) + No, (aq) → Fe* (ag) + No(g) ロ→ロ 」 x g ?
Oxidation-Reduction Equation Balancing in Acidic Solution and Basic
Solution.
Balance the "breathalyze" test reaction in acidic solution, as in example 18.2 on tro C_2H_5OH + Cr_2O_7^2- rightarrow CH_3CO_@H + Cr^3+ Balance in basic solution as in example 18.3 on p Fe(OH)_3 + SnO_2^2+ rightarrow Fe + SnO_3^2-
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+...
Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3. NO−3(aq)+Sn2+(aq)→Sn4+(aq)+NO(g)