Help on 6L.7 part a

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Tiffany Chao 2H
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Help on 6L.7 part a

Postby Tiffany Chao 2H » Tue Feb 25, 2020 9:10 pm

6L.7.a) Write the half-reactions and devise a galvanic cell (write a cell diagram) to study each of the following reactions: AgBr(s) <--> Ag+ (aq) + Br- (aq).
The solutions manual says the half reactions are Ag+(aq) + e- --> Ag(s) and AgBr(s) + e- --> Ag(s) + Br-(aq) but I'm not sure how they were able to get these half reaction equations. I'm not understanding the logic for the pairs (Ag+ and Ag) and (AgBr and Ag and Br-).


Ariel Davydov 1C
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Re: Help on 6L.7 part a

Postby Ariel Davydov 1C » Wed Feb 26, 2020 12:46 pm

Both of these redox reactions can be found in the SRP table on page A16 in the back of the textbook. Since the standard reduction potential of Ag+ + e- -> Ag(s) (0.80 V) is higher than that of AgBr + e- -> Ag + Br- (0.07 V), it will be at the cathode while the latter reaction will be at the anode.

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Re: Help on 6L.7 part a

Postby KnarGeghamyan1B » Wed Feb 26, 2020 2:18 pm

It is based on the equations they give us in the SRP table. You want Ag to cancel since it's not in the original equation, so if you flip the first half reaction, the Ag cancels on each side and you get the original products.

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