For a given reaction associated with an electrochemical cell, K = 0.00134 and Q = 8.75.  Use the dropdowns to generate statements that are true regarding ΔGº, Eºcell, and Ecell for this reaction.   Eocell is...    less or greater than  Ecell

For the voltaic cell described by the cell reaction below, (1) write the cell diagram, (2) identify which specie is being reduced and which is being oxidized, (3) identify the anode and the cathode, (4) calculate the values of Q, and (5) using the table of standard reduction potentials, show the calculation of the Ecell using the Nernst equation [Ecell = E0cell – (0.0592/n x log Q)]. Zn  +  Ni+2 (0.10 M)  →  Zn+2 (0.30 M)  +  Ni

Consider the electrolysis of molten calcium chloride with inert platinum electrodes. The following experimental observations were noted: • Bubbles of pale green chlorine gas are produced at one electrode, Shiny grey molten metallic calcium is produced at the other electrode. Ca2+( ()/Ca(s) E° =-2.84 V Cl2(g)/Cl-(e) E° = 1.36 V Explain what is happening. Your answer should include the following: • The redox processes happening at each electrode. Justify your choice of oxidation and reduction reactions using oxidation numbers and electron transfer. • Movement of the different identified charges. Relating all the observations to the species concerned. Balanced half and full equations. Discussion, with reasons, why this reaction is not spontaneous.

Calculate the K and AG for the following reaction at 25 °C: с Zn(s) + CuSO₂ (aq) = ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °℃ and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. K с Part 2 of 2 = AGO = x10 Round your answer to 4 significant digits. kJ mol X Ś x10

What is the maximum amount of work that is possible for an electrochemical cell where E = 1.58 V and n = 2? (F = 96,500 J/(V･mol))