Consider the galvanic cell: Pt(s) | H2(1 atm)|H*(1 M) || CI'(1 M) | Hg2Cl2(s)|Hg(l) Which of the following changes to the cell would cause the cell potential to increase? O increase the Pt mass decrease the pH O increase the pH O decrease the Pt mass

The free energy change for the following reaction at 25 °C, when [H+] = 1.20 M and [Pb2+] = 3.36x10-3 M, is -38.9 kJ: 2H*(1.20 M) + Pb(s)→ H2(g) + Pb2+(3.36x10-3 M) AG = -38.9 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 v forward reverse

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)| H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for is –0.76 V. (Enter your answer to two significant figures.) pH =

What is the cell reaction for the following voltaic cell? AI(s) | AI³*(aq) || Br"(aq) | Br2(g) | Pt(s) O A(s) + Al3* (aq) → Br (aq) + Br2(g) O AI(s) + 2 Br (aq) → Br2(g) + A13+(aq) O 2 AI(s) + 3 Br2(g) → 2 Al3+ (aq) + 6 Br (aq) O 2 A13* (aq) + 6 Br¯(aq) → 2 AI(s) + 3 Br2(g) O Al(s) + 3 Br2(g) → Al3+(s) + 2 Br (aq)

What is the cell potential of the following cell at 25 oC?       Ni(s) | Ni2+ (1.0 M) || Sn2+ (1.5x10-2 M) | Sn(s)

What is the cell potential at 25oC for the following galvanic cell?   The standard state cell potential (Eocell) is 1.56 V.                                              Zn(s) |  Zn2+ (0.50 M) || Ag+ (2.5 x 10-5 M) | Ag(s)   Select one: a. 1.30 V b. 1.56 V c. 1.95 V d. 1.82 V

The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V. If [Au³+] = 0.50 M, what is the concentration of Cu2+? (R = 8.314 J/K mol, F = 96,500 C.mol-¹) 3Cu + 2Au3+→ 3℃u²+ + 2Au O 1.61 M O1.37 M O 258 M O 5.16 M

Consider the following electrochemical cell: Ag AgNO3(aq) (1 μM)||KCl(aq) (1 µM)| AgCl Ag Calculate the concentrations of all dissolved electroactive species at equilibrium.

4 Consider the voltaic cell: Sn(s) | Sn*2(aq) II Fe*3(aq) | Fe*2(aq) a) Write the overall cell reaction. b) Calculate the standard cell potential at 25°C. c) Calculate the change in free-energy of the reaction at 25°C d) What is the maximum work you can obtain from 25.0 g of nickel? e) What is the value of the equilibrium constant of the reaction? f) Which is the stronger oxidizing agent: Sn*2 or Fe*3? Explain

Gold is frequently purified by electroplating. Typically the gold is dissolved in a cyanide solution (which is fairly selective for gold) and then it is pulled out of solution by electroplating. If the electroplating apparatus used a current of 3.5 amperes, then how long will it take (h) to purify one ounce of gold from a gold(III) cyanide solution? (   You conduct an experiment where you use a single battery with a charge capacity of 900 mAh to precipitate an unknown metal from a salt solution that was leaking from an old battery. You use a vast excess of the salt, so the amount of metal condensed is limited by the battery. You obtain 3.368 g of the metal. You can assume that the metal was the only substance being reduced in the electrochemical cell and 100% of the listed battery charge is usable. If you were able to determine that the metal ion was a +2 ion, then which metal is it? This metal was used in batteries for a long time (even in “alkaline” batteries) due to its good…