a. In Ag2S , Ag remains in +1 oxidation state but upon reaction it becomes elementary Ag, having oxidation state 0 (zero). So, upon reaction Ag+ gets reduced to Ag. Again on the other hand, Al before reaction was in elementary state, having oxidation state 0, but after reaction it goes to +3 in Al2S3. So, Al gets oxidized to Al3+ due to reaction. We, know, the reduction occurs in cathode and oxidation occurs in anode, so here Ag2S is acting as cathode and Al is acting as anode.
Tips for oxidation state calculation:
i. Overall molecule has oxidation state zero
ii. Consider sulpher having oxidation state -2 per atom
So, for Ag2S, if oxidation state per Ag atom is x, then,
Similarly for Al2S3,
b. From the reaction given above and the observations, it is clear that, the reaction is highly spontaneous. The reaction started just after adding the neckless into the bowl. So, from the knowledge of therrmodynamics we can say for the reaction is highly negative. Now, from the knowledge of electrochemistry we know, . n stands for no of electron transferred in the process, F is Faraday constant and they both are positive. The term left is the ECell , i.e, the cell potential for the electrochemical cell formed in the reaction medium. In order to make negative, Ecell must be positive. So, under the reaction condition, Ecell is highly positive.
c. If 32 Al atoms reside there, then the number of Al2S3 molecule there is 16. Molar mass of Al2S3 is
. In 1 mole of molecule there are Avogadro number of molecules, i.e, molecules.
Now, 1 angstrom = 10-8 cm, so actual volume is
Now, density = (mass) / (volume), thus,
A student is attempting to reverse the tarnishing (silver sulfide, Ag2S(s), formation) on her silver necklace using a method she found online. She lined a bowl with aluminum foil, added some baking s...