Question

Exercises Predict which of the following will react spontaneously in the standard state. Keep in mind that not all reactions are oxidation-reduction. Write balanced net ionic equations for reactions which occur. If no reaction occurs in the forward direction, write "no reaction". 1. H2(g) + Ag*(aq) 2. r(aq) + Zn2+(ag) 3. Cl(aq) + Agt(ag) 4. Fe2(aq) + MnO4 (aq) (in acidic solution)

Answer 1

Answers Gillen, o predict which of the following will react Spontaneously in the standard state, keep in mind that not all reactions are onidation -reduction. o write balanced net ionic Equations for reactions Which occur. o if noteaction direction occurs in the forward write "no reaction" (1) H2(g) + Ag+ (aq) Now Compare reduction potentials: Ag + te = Ag(3] +0.7996; 2H+ + 20 = H210) 0.0 Clearly, Ag is likely to form Ag(s) Therefore, This will be spontanoves net ionic H2(g) + Ag + laq) Ag(s) + 2H+lag) net ionic balanced. H2(g) + 2Agilaq )->2Ag (s) + 2H+ (aq)

2. Tlaq) + Zu?+(aq) Compowe reduction potentials: 12 (3) +20 21-+0.54 Zn2+ + 2e- z znis) - 0.7613 Clearly, I is likely to remain as I Zn is not likely to form Zn ,' therefore, "No reaction" 3 a laq) + Agtlaq) here, Agcals) is not scluble Agce(s) t Ag+ 4Cl- will occurs to a very Entent, this is not likely to be spontaneous low Therefore, there is no reaction" I Feltlaq) + Mnori (aq) [in acidic Solution] Here, Fe2+ + 200 - Fels)-0.44 Mnon- + 8H+ -5e = Mn2+ + +H 20 +1:57

Creally, Mhow is likely to educe, where as Fet2 is likely to be onidized. This is not likely to occur Therefore, No reaction will take place |