Calculate the pH of cathode half-cell solution if the cell emf at 298 K is measured to be +0.684 V when [Zn2+]=0.30 M and Ph2=0.90 atm

A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a solution containing 1.00 M Sn2+ and 1.00 M Sn4+. The other half-cell has a thallium rod immersed in a solution of 1.00 M Tl+. What is the equilibrium constant at 25° C?(Eo= Tl+ / Tl = −0.34 V.)? What is the cell voltage if the Tl+ concentration is increased 6−fold?

A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?

Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V