Aluminum can replace copper ions in solution. Use the following table to answer this item. Reaction E° (V) Reaction E (V) F2 + 2e¯ –→ 2F¯ 2.866 Cu²+ + e¯ → Cu+ 0.153 4+ 2+ H2O2 + 2H* + 2e¯ → 2H2O 1.776 Sn + 2e¯ → Sn“ 0.151 AgBr + e 2H* + 2e¯ –→ H2 N20 + 2H* + 2e¯ → N2 + H,O 1.766 → Ag + Br 0.07133 Au+ + e¯ –→ Au 1.692 0.0000 MnO4 + 4H† + 3e¯ → MnO2 + 2H3O 1.679 Fe3+ + 3e¯ → Fe -0.037 2D* + 2e¯ –→ D2 -0.044 HСIO, + H* + Зе — Cl2 + 2H,O Mn+ + e¯ → Mn²+ 1.63 Pb2+ + 2e¯ → Pb -0.1262 Sn²+ + 2e¯ → Sn -0.1375 1.5415 Ni?+ + 2e¯ → Ni -0.257 MnO4 + 8H* + 5e° Mn²+ + 4H2O 1.507 Co²+ + 2e¯ → Co -0.28 PBSO4 + 2e¯ → Pb + SO4²¬ Cr+ + e¯ → Cr²+ -0.3588 Au³+ + 3e¯ → Au 1.498 -0.407 Cl2 + 2e¯ → 2 Cl¯ O2 + 4H† + 4e 1.358 Fe2+ + 2e¯ → Fe -0.447 → 2H2O 1.229 Cr³* + 3e¯ → Cr -0.744 Br2 + 2e 2H9²+ + 2e¯ → Hg2² Hg²+ + 2e Ag* + e¯ → Ag Hg, → 2Br 1.087 Zn²+ + 2e¯ → Zn -0.7618 2+ 0.920 2H2O + 2e¯ → H2 + 20H- Cr2+ + 2e¯ → Cr -0.8277 → Hg 0.851 -0.913 0.7996 Al³+ + 3e¯ –→ Al -1.662 2+ + 2e → 2Hg 0.7973 Be2+ + 2e¯ → Be -1.847 Fe+ + e → Fe2+ 0.771 Н, + 2е — 2H -2.23 MnO4 + e¯ → MnO4²- 0.558 Mg²+ + 2e¯ –→ Mg - 2.372 I3 + 2e¯ -→ 3I¯ 0.536 Na* + e –→ Na -2.71 I2 + 2e → 21- 0.5355 Ca2+ + 2e¯ → Ca - 2.868 Cu* + e¯ –→ Cu 0.521 Lit + e → Li - 3.04 O2 + 2H2O + 4e¯ → 40H- Cu²+ + 2e 0.401 → Cu 0.3419 Hg,Cl, + 2e¯ → 2Hg + 2CI- 0.26828 AgCl + e¯ → Ag + Cl¯ 0.22233 True O False

Balance the following reaction in acidic solution. Fe?+ (ag) + MnO, (aq) → Fe+ (ag) + Mn²+(aq) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. Fe2+ + MnO,¯ + 4 Fe3+ + Mn2+ +

Consider the redox reaction shown below: IO3-1(aq)    +  5 I-1 (aq)   +   6 H+1 (aq)   →   3 H2O (l)   +   3 I2 (aq) What is the reducing agent?

10. Balance the following redox reaction using the half-reaction method and tell how many electrons are transferred in the reaction. Ag(s) + CN (aq) +O2 (g) → Ag(CN), + H2O (BASIC medium) HINT: CN- is neither oxidized nor reduced

The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. Co2+ + NO  Co + NO3-

The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction is given below. 2 H2O(l) + 2 e− → H2(g) + 2 OH− (aq) Hydroxide ion reacts with lactic acid as soon as it is produced. The endpoint of the reaction is detected with an acid-base indicator. It required 104 s for a current of 13.1 mA to reach the endpoint. How many grams of lactic acid (a monoprotic acid) were present in the sample?

In the balanced redox reaction: 2 Cu(s) + S(s) > Cu 2S(s); how many electrons are gained or lost by each copper atom?

In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction. 2NO(g)+O2(g)⟶2NO2(g)

Predict which species will be oxidized and which will be reduced in a molten salt mixture that contains CdI2, NaOH, and AlCI3. Cd2+(aq)  +  2e  →  Cd(s)                                        Eored = – 0.40 V I2(s)  +  2e  →  2 I–(aq)                                            Eored = + 0.54 V Na+(aq)  +  1e  →  Na(s)                                         Eored = – 2.71 V Cl2(g)  +  2e  →  2 Cl–(aq)                                       Eored = + 1.36 V Al3+(aq)  +  3e  →  Al(s)                                          Eored = – 1.66 V O2(g)  +  2 H2O(l)  +  4e  →  4 OH–(aq)                  Eored = + 0.40 V     which is oxidized    which is reduced

/variants/1189727/take/9/ ☆ 88 MULTIPLE CHOICE Question 10 Which half-reaction correctly represents oxidation? Fe(s) → Fe +2 A Fe(s) B Fe +2 (aq) + 2e¯ (aq) → Fe(s) + 2e- + 2e → Fe+2 (ag) D Fe +2 (aq) + 2e¯ → Fe(s)