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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: bradenator on June 14, 2021, 10:53:59 PM

Title: Cell Potentials
Post by: bradenator on June 14, 2021, 10:53:59 PM

I have no idea what I should use as the reduction potential for   Mn—>Mn(NO3)2 or       Sn(NO3)2—>Sn

I can’t find these on the reduction potential table.

Title: Re: Cell Potentials
Post by: Borek on June 15, 2021, 02:49:58 AM

Nitrates are dissociated, what ions will be present in the solution?

Title: Re: Cell Potentials
Post by: bradenator on June 15, 2021, 12:03:41 PM

Quote from: Borek on June 15, 2021, 02:49:58 AM

Nitrates are dissociated, what ions will be present in the solution?

Would it just be Mn^2+ and Sn^4+? How would I know which side of the reaction these ions go on?

Title: Re: Cell Potentials
Post by: bradenator on June 15, 2021, 01:13:38 PM

Quote from: Borek on June 15, 2021, 02:49:58 AM

Nitrates are dissociated, what ions will be present in the solution?

I believe I have figured it out. Is it 1.049?

Title: Re: Cell Potentials
Post by: Orcio_87 on June 15, 2021, 05:35:33 PM

Quote

I believe I have figured it out. Is it 1.049?

Do you mean standard potential of:

Mn + Sn²⁺ ---> Mn²⁺ + Sn

?

Slightly lowered, but it is OK.

Maybe source of data gives this little difference (about 0,005 eV).

Title: Re: Cell Potentials
Post by: bradenator on June 15, 2021, 09:02:52 PM

Quote from: Orcio_Dojek on June 15, 2021, 05:35:33 PM

Quote

I believe I have figured it out. Is it 1.049?

Do you mean standard potential of:

Mn + Sn²⁺ ---> Mn²⁺ + Sn

?

Slightly lowered, but it is OK.

Maybe source of data gives this little difference (about 0,005 eV).

Yeah that’s what I got. Thank you for confirming for me!