A galvanic cell is made ot a Ni2*/Ni halt cell with [Ni2 | = 6.00 x 10-2 M and an Ag"/Ag half cell with [Ag"] = 4.00 x 10 M. Calculate the electromotive force of the cell at 25 °C. The reduction potentials for the two half reactions: Ni2+ (aq) + 2e →Ni(s) Ag*(aq) + e¯ →Ag(s) E° = -0.24 E° = +0.8 O a. 1.14 O b. 0.64 O c. 1.04 O d. 1.06 O e. 0.94

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V

Use the standard reduction potentials given below to predict if a reaction will occur when Mg metal is put into a 1 M aqueous Cd²+ solution. Cd(s) Eº = -0.403 V red Eº → Mg(s) Fred = -2.370 V Cd2+ (aq) + 2e → 2+ Mg²+ (aq) + 2e If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- →  La (s)     E° = -2.37 V Na+ (aq) + e- → Na (s)         E° = -2.71 V       1.8 x 10-6     5.7 x 10-18     5.6 x 105     1.7 x 1017