Question

Q1:

a) Describe how a galvanic cell works and include a fully labelled sketch. Explain clearly what is occurring in each ‘side’.

b) You add Mg to a beaker containing HCl(aq) and a gas is produced. Explain, chemically, what is happening and write a balanced equation for the reaction, including how many electrons are transferred. How could you harness the reaction to do useful work?

c) The equation ΔG^o = -nFE^o is also applicable to half-reactions. Using standard reduction potentials, estimate ΔG^o_f for both Fe²⁺(aq) and Fe³⁺(aq).

Answer 1

Explanation of galvenic cell structure, diagram, working mechanism

- soul Salt Bridge Anode (zine) eeeathode (Copper) - Poroas plug- euson solution ansou solution Fig. Gelanie cell Galvomie eell- A galvanie cell converts chemical energy to electrical energy. The cell consists Ar two electrods immersed in mu one or more suitable electreolytes the electrodes are externally conected through a copper wine and internally through ac salt bridge, then a chemical reaction oeeum in the cell envolving. al oxidation at one electre ade and reduction at the other electrod. In which onidation occure is called the anode and in which reduction ocunes is called eathode. The metal of the mode will oncidize , going from an anigation state of o(zero) to a positive oxidation state, and it will become an ion # that time At The cathode the metal ion in the solution will accept one One more in electrons from the cathode and the ions onidation state will reeduce to o(zero) this tom form a solid metal that deposite on the cathode... When the electrons that leave the metal of the mode and through the wine to cathod, the Amiter shows reeflection The flow of electrons is an cleetrical eurment which can be used to do work. The reactions are shown below - Anode - En Zn2+ + 2e- overal cathode - eu2+ + 2e eu, 2n(s) + ext (aq) → 22 + (aq) + Curs)