Calculate Eo, E, and ΔG for the following cell reactions (a) Mg(s) + Sn2+(aq) ⇌ Mg2+(aq) + Sn(s)      where [Mg2+] = 0.045 M and [Sn2+] = 0.050 M   (b) 3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s)     where [Cr3+] = 0.020 M and [Zn2+] = 0.0065 M

The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M)     ΔG = 68.1 kJ What is the cell potential for the reaction as written under these conditions? Answer:  V Would this reaction be spontaneous in the forward or the reverse direction?

Give the standard line notation for each cell. (a) 2 IO3¯(aq) + 10 Cr²+ (aq) + 10 H+ (aq) ⇒ 10 Cr³+(aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Cr²+ (aq), IO3¯(aq), H+ (aq) || Cr³+ (aq), I2 (aq) | Pt(s) Pt(s) | Cr³+ (aq), I2 (aq) || Cr²+ (aq), 103¯(aq), H+ (aq) | Pt(s) Pt(s) | IO3¯(aq), H+ (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) Pt(s) | Cr²+ (aq), Cr³+ (aq) || IO3¯¯(aq), H† (aq), I₂ (aq) | Pt(s) (b) (c) (d) Co(s) + 2 Ag+ (aq) ⇒ Co²+ (aq) + 2 Ag(s) Co(s) | Ag+ (aq) || Co²+ (aq) | Ag(s) (aq) || Ag* (aq) | Co(s) Ag(s) | Co²+ 2+ Ag(s) | Ag+ (aq) || Co²+ (aq) | Co(s) 2+ Co(s) | Co²+ (aq) || Ag+ (aq) | Ag(s) H2O2(aq)+2 H*(aq)+2e O₂(g) + 2 H+(aq) + 2 e¯ → H2O2(aq) Pt(s) | H₂O₂ (aq) | 02 (9) || H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq) | Pt(s) Pt(s) | H₂O2 (aq), H+ (aq) || O2(g) | H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | O2(g) | H₂O2 (aq), H† (aq) || H₂O2 (aq), H† (aq) | Pt(s) 00 Mn²+ (aq) + 2 e → Mn(s) → 2H,O(l) 3+ Fe³+ (aq) + 3 e → Fe(s) Eº E° -1.18 V 3+ Fe(s) | Fe³+ (aq) || Mn²+ (aq) | Mn(s) Fe(s) | Mn²+ (aq)…

3. Calculate the standard potentials for each of the cells at 298 K. Is each combination spontaneous as written? (a) Ag (s) | Ag + (aq) || Au *3 (aq) | Au (s) (b) Cu (s) | Cu +2 (aq) || Al *3 (aq) | Al (s)

A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.

Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)

If an alkaline battery produces a cell potential of 1.66 V, what is the value (in kj) of ΔGcell? The half-reactions in alkaline batteries are: ZnO(s) + H2O(l) + 2e^-  --------> Zn(s) + 2OH^- (aq) 2MnO2(s) + H2O(l) + 2e^-  -----------> Mn2O3(s) +  2OH^- (aq)

For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g)        ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)      ?o=−0.403 V   Calculate the H+ concentration in M.

An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: Pt|I2, I- O Mg²+|Mg cathode: O Pt|I2, I- Mg2+|Mg (b) What is the emf of the cell? 4.0 2.869 X V (c) What is the spontaneous cell reaction? chemPad OHelp Greek - Mg2+(aq)+21 (aq) Mg(s)+I2(aq) Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq) Your answer appears to have inconsistent states-of-matter. (d) What is the equilibrium constant of the cell reaction? 2.42e98

Use the tabulated half-cell potentials to calculate ΔG° for the following reaction. (Hint: Before you being, you must determine whether or not the reaction is balanced.)I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq) (a)‒1.1×102kJ (b) +4.9×101kJ (c) ‒9.7×101kJ (d) ‒3.3×102kJ