What is the Ecell for the following cell at 25°C? Pt Sn2+ (0.233 M), Sn4+ (1.05 M) || Ag*(2.22 x 10-2 M) | Ag E° = 0.800 V Ag++e-→Ag(s) Sn4+ +2 e- → Sn2+ E° = 0.154 V A) 0.529 V B) 0.763 V C) 0.680 V D) 0.578 V E) 0.412 V

Using the data provided below, calculate the emf, E°, for the following cell at 25°C. Ni(s)|Ni2+(1.20M)||Sn2+(1.0x10-4M)|Sn(s) Express your answer to two decimal places.   Sn2+(aq) + 2e- ----> Sn(s)        E° = -0.136 V Ni2+(aq) + 2e- ----> Ni(s)          E° = -0.28 V

What is e cell of the following electrochemical cell ag(s) / agcl (s), KCl (aq, 1 M) // H2 (g, 1 atm), pH 7.00 aq / Pt (s)

What is the pH in the cathode for the following galvanic cell made from the following two half reactions? The initial concentration of gold ion is 1.1x10-3 M, the initial concentration of permanganate is 6.42 M, and the Ecell is 0.15 V. Assume the temperature is 298K. Au3+(aq) + 3e- →   Au(s)                                     E° = 1.52 VMnO4-(aq) + 4H+(aq) 3e- → MnO2(s) + 2H2O(l)      E° = 1.70 V