(1) Define the following terms: faraday, salt bridge, anode, cathode, voltaic ce
ID: 592230 • Letter: #
Question
(1) Define the following terms: faraday, salt bridge, anode, cathode, voltaic cell, electrolytic cell. (2) Consider the following galvanic cell: Pt -Ni Ni2+ (a) Identify the anode and cathode. (b) Write the balanced equation for the cell reaction. (c) Write the shorthand notation (also known as the cell diagram) for the cell. (3) Calculate the cell potential, the equilibrium constant, and the free-energy change for Ca (s) + Mn2+ (aq) ( 1 M)Ca2+ (aq) ( 1 M) + Mn (s) given the following E° values: Ca2+ (aq) + 2e- Ca (s) Mn2+(aq) + 2e- Mn (s) E--2.87 v E118 V (4) Arranging Oxidizing and Reducing Agents in Order of Increasing Strength (a) Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: (b) Arrange the following reducing agents in order of increasing strength under standard-state conditions Al(s), Na(s), Zn(s).Explanation / Answer
Q1.
Faraday --> amount of charge per unit mol of electron
Salt bridge --> brige between eletrolytic cells which allow ion flow
anode --> electrode in which oxidation, loss of electrons, is done
cathode --> electrode in which reduction, gain of electrons, is done
voltaic cell --> a cell which consist of two half cells, each consisting in reduciton and oxidation. Electirc charge is produced
eletrolytic cell --> cell similar to voltaic clel, but in this cae electricity is applied, in order to favour a reverse reaction
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