You wish to construct a galvanic cell with the anode consisting of a Ni electrode in a 1.0 M Ni(NO3)2 solution. Which of the following would give you the highest standard cell potential if used as the cathode in this galvanic cell? a.) Sn4+(aq) + 2e− →Sn2+(aq)      Eo = +0.13 V b.) Cu2+(aq) + 2e− →Cu(s)            Eo = +0.34 V c.) Fe2+(aq) + 2e− →Fe(s)             Eo = −0.44 V d.) Au3+(aq) + 3e− →Au(s)            Eo = +1.50 V

Q: Consider the galvanic cell shown below (the contents of each half-cell are written beneath each…

A: This question can be solved via nernest equation. In the above question half cell reactions are…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr (aq)…

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2     E0= -2.87…

Q: Under standard conditions, the cell potential for a voltaic cell composed of zinc and copper is 1.10…

A:

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Given Reactions: O2 (g)+ 4 H+ +4 e- ------> 2H2O                                 Eored=  +1.23 V…

Q: a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc…

A:

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.