# Problem: Balance each skeleton reaction, use Appendix D to calculate E°cell, and state whether the reaction is spontaneous:(b) AgCl(s) + NO(g) ⟶ Ag(s) + Cl−(aq) + NO3−(aq) [acidic]

###### FREE Expert Solution

We are asked to balance the redox reaction under acidic conditions: AgCl(s) + NO(g) ⟶ Ag(s) + Cl(aq) + NO3(aq)

*Before balancing the redox reaction:

ignore H+, OH-, and H2O in the starting reaction

Step 1: Separate the whole reaction into half-reaction

AgCl(s) →  Ag(s) + Cl(aq)                                                 NO(g)→ NO3(aq)

Step 2: Balance the non-hydrogen and non-oxygen elements first

AgCl(s) →  Ag(s) + Cl(aq)                                                 NO(g)→ NO3(aq)

Step 3: Balance oxygen by adding H2O(l) to the side that needs oxygen (1 O: 1 H2O)

AgCl(s) →  Ag(s) + Cl(aq)                                               NO(g) +2 H2O (aq)→ NO3(aq)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)

AgCl(s) →  Ag(s) + Cl(aq)                                               NO(g) +2 H2O (aq)→ NO3(aq) + 4 H+(aq)

Step 5: Balance the charges: add electrons to the more positive side (or less negative side)

AgCl(s) +1 e-→  Ag(s) + Cl(aq)                                 NO(g) +2 H2O (aq)→ NO3(aq) + 4 H+(aq) + 3 e-

Step 6. Balance electrons on the two half-reactions

▪ multiply the reactions so both half-reactions have the same number of electrons

▪ electrons should cancel in the overall reaction

[ AgCl(s) +1 e-→  Ag(s) + Cl(aq)   ]   x 3

NO(g) +2 H2O (aq)→ NO3(aq) + 4 H+(aq) + 3 e-

Step 7. Get the overall reaction by adding the two reaction.

species that appear in both reactions on opposite sides are subtracted

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###### Problem Details

Balance each skeleton reaction, use Appendix D to calculate E°cell, and state whether the reaction is spontaneous:

(b) AgCl(s) + NO(g) ⟶ Ag(s) + Cl(aq) + NO3(aq) [acidic]