Calculate the theoretical cell potential for the following galvanic cell:                  Zn | Zn2+ (1 M) || Mg2+ (2 M) | Mg

Consider a galvanic cell based on the reaction   2 Fe2+ (aq)     +   Cl2 (g)   ------------>2 Fe3+ (g)    +          2Cl- (aq)   Calculate the cell potential at 25oC when [Fe2+  ] =1.0 M,  [Fe3+ ] = 1.0 x 10-3 M,  [Cl- ] = 3.0 x 10-3 M and PCl2 = 0.50 atm.

Use the standard half cell potentials listed below to calculate the standard cell potential for the following reaction that occurs in an electochemical cell at 25 ° C.

Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Eof this galvanic cell. cell 5.939 V 3.158 V 2.899 V 2.899 V O - 5.939 V

What is the standard cell potential for the voltaic (galvanic) cell using the following half-cell reactions with the indicated standard half-cell potentials: Be²⁺(aq) + 2e⁻→Be(s), E⁰ = -2.9V and Cl₂ + 2e⁻→2Cl⁻(aq), E⁰= +1.4 V A) -1.5 V B) +1.5 V C) -4.3 V D) 4.3 V

|| Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 0 2+ 2+ Cu (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.39 M Cu in one half-cell and 2.14 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ

For the galvanic cell  2Ag+ + Cr  →  2Ag + Cr2+,  which equation allows you to correctly calculate the standard cell potential?

. Calculate ΔG ̊for the following reaction if the standard cell potential is 1.02 V: Cu(s) + Cl2(g) → Cu2+(aq) + 2Cl–(aq)

A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M tin(IV) ion and 1.0M tin(II) ion, and another inert platinum clectrode in a solution containing 1.0 M iron(III) ion and 1.0M iron(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. E: cell V

Calculate the cell potential, G (J), and the equilibrium constant Keq for the followingelectrochemical cell and determine the spontaneous reaction direction.Pb(s) | Pb2+ (1.50 x 10-5 M) || Cr2O7 2-(0.150 M), Cr3+ (0.250 M), H+ (0.010 M) | Pt(s)