The standard potential for the reaction below is 0.203 V at 25°C. 3 Y+4 (aq)  + 4 X (s) →  3 Y (s) +  4 X+3 (aq) Calculate the value of the equilibrium constant for the reaction at 25°C.

A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a cell potential of 0.763 V. Calculate the maximum electrical work generated when 17.0 g of zinc metal is consumed. Maximum electrical work-

Balance the following reaction. Calculate the cell potential and the Gibbs free energy of the reaction at standard conditions. Write the line representations for the Galvanic cells, indicating the anode and cathode.

How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten CaCl2?

Calculate the equilbrium constant, K, for the reaction

Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Cu²+ (aq) = Ti²+ (aq) + Cu(s) 2+ 2+ occurs at 25 °C, given that [Ti 1= 0.00130 M and [Cu]=0.892 M. Refer to the table of standard reduction potentials. E=

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Cu²+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ Suppose the cell is prepared with 5.43 M Cu²+ in one half-cell and 3.33 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 X μ 00 Ś

Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K.   Cd2+(aq) + 2e–   →  Cd(s)                     E° = –0.403 V                         Pb2+(aq) + 2e–   →   Pb(s)                     E° = –0.126 V     E°cell = ______________     Ecell = ______________

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn (aq)+Ba (s) Sn (s)+ Ba" (aq) 2+ Suppose the cell is prepared with 4.24 M Sn 2+ in the other. in one half-cell and 2.000 M Ba' Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (pH2)= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.200 V, what is the pH of the unknown solution at 298 K?