Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. 2NO(g) + 4H₂O (/) + 3 Br₂ (1) 2NO, (aq) +8H' (aq) +6Br (aq) 1 Du 0.8

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --

Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);

Using standard reduction potentials from the ALEKS Deta tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. Cu (aq) + HNO₂ (aq) + H* (aq) → Cu² (aq) + NO(g) + H₂O (1) X