Pt(s) |X*(ag), X2+, ELECTROCHEMISTRY: Pt(s) |X"(aq)» Given the line notation: (aq) || Y3+ (aq) IY(s) where: x2+ + e → x* E° = 0.94 V y3+ + 3 e¯ → Y E° = -2.71 V Pt4+ + 4 e → Pt E° = 1.20 V Calculate the EMF.

Given the following reactions, AgBr(s) 2 Ag*(aq) + Br (aq) Ag (aq) + 2 CN (aq) 2 Ag(CN)2 (aq) Ksp = 5.8 x 10-13 Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN (aq) ZAg(CN), (aq) + Br (aq)

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Calculate ΔG° for the redox reaction represented by the cell diagram       Pt(s) | Cl2(g, 1 atm)  || ZnCl2(aq, 1 M) | Zn(s).

Calculate the EMF of the following electrochemical cell: Pt | VO2+(0.25 M), V3+(0.10 M), H+ (0.001 M) || TI3+ (0.10 M), TI+(0.05 M), | Pt Indicate whether the cell is galvanic or electrolytic. Evo2+/v3+ = 0.361 V, ET³+/T+ = 1.25 V   Ans: 1.23 V, galvanic

9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?

What is the balanced reaction for the following galvanic cell?Cr(s)| Cr3+(aq) || Fe3+(aq) | Fe(s)   Fe(s) + Cr(s) ↔ Fe3+(aq) + Cr3+(aq)   Fe3+(aq) + Cr3+(aq) ↔ Fe(s) + Cr(s)   Fe3+(aq) + Cr(s) ↔ Fe(s) + Cr3+(aq)   Fe(s) + Cr3+(aq) ↔ Fe3+(aq) + Cr(s)

At a temperature of 25 ° C the galvanic element Pt | MnO4- 0,10M, Mn2 + 0,1M, pH = 1 | Ag + 0.0001M | Ag has the electromotive force 0,80V. Calculate the standard electrode potential of Ag + if E ° (MnO4 -, H + | Mn2 +) = 1.50V

For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M), Cr2+(aq)(.301M)|Pt(s) Determine the cell potential for this electrochemical cell by first calculating the standard cell potential and then by using the Nernst equation.

AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.