Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol

Calculate Eº, E, and AG for the following cell reaction: 2+ 2+ Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s) 2+ 2 where [Mg²+] = [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers to 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10ª Part: 0 / 3 Part 1 of 3 Eº = v V x10 J V. mol S I

Consider the electrolysis reactions cathode anode whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = Cu²+ (aq, 0.177 M) +2e=Cu(s) H₂O(1) ⇒ 10₂(g, 1 bar) + 2 H+ (aq, 0.195 M) + 2 e¯ The cell has a resistance of 66.0 and a current of 7.17 mA when the cathode overpotential is 0.231 V and the anode overpotential is 0.050 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Ecell = V V

Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś

The standard state cell potential for the reaction below is 1.030 V. Zn(s) + Hg,Cl,(s)→ ZnCl,(aq) + 2Hg(1) Calculate the standard state Gibb's energy change (in kJ) at 298K for the reaction. O -99.4 kJ O -199 kJ O 199kJ O 99.4 kJ

Determine the cell potential for the following cell Ni(s) | Ni2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Ni2+(aq) and Ag+(aq) are –0.25 V and +0.80 V, respectively.   A.  1.05 V   B.  1.10 V   C.  1.00 V   D.  1.16 V   E.  0.94 V

The standard cell potential for the reaction shown here is .653 V. Calculate the cell potential at 25°C with [Hg^2+] = 0.0500 M, [V^2+] = 0.100 M, [Hg2^2+] = 0.00500 M and [V^3+] = %3D 0.0200 M. [Hg?+] do.o500 M [V2+] = 0.100 M H0.0500 M [Hg* = 0.00500 M [V³*] = 0.0200 M 2 Hg²+ (aq) + 2 V²+ (aq) = Hg2²+ (aq) + 2 V³+ (aq)