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- What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 VThe reaction Cr(NH3)6*(aq) + 3en(aq) --> Cr(en)3+*(aq) + 6 NH3(aq)where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction. the reaction is spontaneous for all temperatures. the reaction is spontaneous for low temperatures. the reaction is non-spontaneous for all temperatures. the reaction is spontaneous for high temperatures. not enough info to tell.Write the balanced net ionic equation for the reaction of aqueous sodium sulfate with aqueous lead(II) nitrate. Include phases. net ionic equation: Pb2+ (aq) + S²- (aq) PbS(s) Incorrect SPECIAL ΔΣΩ λμπ x"| Xo EX| (s) (1) || (aq) (g) () [] CLR
- Give the standard line notation for each cell. (а) 2 IOз (аq) + 10 Cr (аq) + 10 H* (аq) — 10 Cr" (ag) + I2(ад) + 5 Нә0(1) O P(:) | Cr* (a), I> (aq) || Cr?* (аg), IO; (ад), н (аg) | Pt(s) O Pe(s) | Cr* (ag), IO; (ад), Н* (аq) | Cr* (aq), Iz (aq) І Pt(s) "(aд), I2 (aд) | Pt(8) O P(6) | 10; (aд), н* (аq), 1ә(аq) | Cr?* (ag), Cr** (ag) | Pt(6) Pe(s) | Cr* (aq), Сr* (aq) || IOз (aд), H* (ад), I2 (ад) | Pt(8) (b) Zn(s) +2 Ag* (aq) = Zn?+ (aq) + 2 Ag(s) O Ag(s)| Zn²+(aq) || Ag* (aq) | Zn(s) O Ag(s)| Ag*(aq) || Zn²+ (aq) | Zn(s) Zn(s) Ag* (ag) || Zn?+ (ag) | Ag(s) Zn(s) | Zn²+ (aq) || Ag* (aq) | Ag(s) (c) Н;О2(ад) + 2 H* (аq) + 2 е 2 Hә0(1) E° 1.78 V О:(9) + 2 H (аq) + 2 е — Н,O%(аq) E° = 0.68 V O P(8) | H2О2(ад) | Pt(8) O Pt(s) | O2(9) | H,O2 (aq), H† (aq) || H,O2 (aq), H† (aq) | Pt(s) Pt(:) | H>О2(аq) | 02(9) || н* (аq) | Pt(8) O Pe(8) | H2О2(аg), H* (ад) || О2 (9) | Н-О2(ад), Н* (ад) | Pt(s)In Al + FeO --> Al2O3 + Fe what is the coefficient for Fe ?Predict whether the following reactions will be spontaneousin acidic solution under standard conditions:(a) oxidation of Sn to Sn2+ by I2 (to form I-), (b) reductionof Ni2+ to Ni by I- (to form I2), (c) reduction of Ce4+ to Ce3+by H2O2, (d) reduction of Cu2+ to Cu by Sn2+ (to form Sn4+).
- ensider the following equilibrium: Cu2+, *(aq) + 4NH3(ag)=Cu(NH3)42+ (Kf = 4.8e+12) (ag) solution is made by mixing 18.0 mL of 1.50 M Cuso, and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. Please e Formation Equilibrium Constant for assistance. What is the concentration of NH3 in the resulting solution? [NH3] = What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3),2+] = M What is the concentration of Cu2+ in the resulting solution? [Cu²+] = | M4. When considering the species: K (s), K* (aq), Au (s), Au* (aq), I2 (g), and I- (aq), the strongest reducing agent would be: (a) K (s) (b) K+ (aq) (c) Au (s) (d) Au3+ (aq) (e) I2 (g) (f) I- (aq)(a) A Cr3+(aq) solution is electrolyzed, using a current of7.60 A. What mass of Cr(s) is plated out after 2.00 days?(b) What amperage is required to plate out 0.250 mol Crfrom a Cr3+ solution in a period of 8.00 h?
- Which species in each pair is a better oxidizing agent under standard-state conditions? a) Brz or Au, b) Hz or Ag+, c) Cd or Cr", d) Oz in acidic media or Oz in basic media. Given that: Br2(1) + 2e 2Br(aq) Au (aq) + 3e Au(s) H2(g) + 2e 2H*(aq) Agʻ(aq) + e- → Ag(s) Cd*(aq) +e → Cd(s) O,(g) + 4H + 4e → 2H,0(1) O(g) + 2H,0(1) + 4e → 40H(aq) E° = +0,40 V E° = +1,07 V E° = + 1,50 V E° = - 2,25 V E° = +1,98 V E° = - 0,40V E° = + 1,23 VWhen Cr(III) is oxidized to Cr(VI), its solubility, mobility and toxicity are dramatically increased.Given the following data:log KFe(OH)3(s) + e- (aq) + 3H+ (aq) = Fe2+(aq) + 3H2O(l) 16.720.33HCrO4-(aq) + e- (aq) + 1.33H+ (aq) = 0.33Cr(OH)3(s) + 0.33H2O(l) 18.81(a) What is the oxidation state of Fe in Fe(OH)3?(b) Determine if Fe(OH)3 may oxidize Cr(III) in solid Cr(OH)3 under standard conditions34. A galvanic cell is constructed in which the overall reac- tion is Cr,O (aq) + 14 H0 (aq) + 61 (aq) –→ 2 Cr" (aq) + 3 12(s) + 21 H,O(() (a) Calculate AE for this cellI. (b) At pH 0, with [Cr,O ] = 1.5 M and [I] = 0.40 M, the cell potential is found to equal 0.87 V. Calculate the concentration of Cr*(aq) in the cell.