# For the following electrochemical cell co(s)|co2 (aq. 0.0155 m)||ag (aq. 3.50 m)|ag(s)

For the next electrochemical
cell Co(s)|Co2 (aq,
0.0155 M)||Ag (aq, 3.50 M)|Ag(s)
For the next electrochemical
cell Co(s)|Co2 (aq,
0.0155 M)||Ag (aq, 3.50 M)|Ag(s)

For the next electrochemical cell Co(s)|Co2+(aq, 0.0155 M)||Ag+(aq, 3.50 M)|Ag(s) write the web cell equation. Section are non-compulsory. Don’t embody the concentrations. Calculate the next values of 25.0 diploma C utilizing customary potentials as wanted.

Common steerage

Ideas and cause
Within the cell notation, the oxidation half response on the left of the salt bridge is that of the anode and the discount half response on the precise of the salt bridge is that of cathode.
The idea used to calculate the cell potential is Nernst equation. It’s as follows:

Right here, n is the variety of electrons transferred.
The relation between and is as follows:

Right here, n is the variety of electrons transferred and F is Faraday fixed.

Fundamentals

Cell notation is a brief type of the anode and cathode half reactions which are going down in an electrochemical cell. The double vertical bar within the cell notation represents the salt bridge.

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Step-by-step

Step 1 of three

The given cell notation is,

The reactions which are going down at anode and cathode are as follows:

Subsequently, the web cell response is .

The online cell response is .

Earlier than including the 2 reactions, multiplied the cathode response with 2 to steadiness the electrons within the two half reactions.

Ensure that the electrons within the two half reactions have cancelled one another by including the 2 reactions.

Calculate the of the response from the usual discount potentials.

Step 2 of three

The discount potentials of the 2 half-reactions are as follows:

Calculate from as follows:

The and are as follows:

The variety of electrons modified within the response is 2. Therefore, 2 is substituted for n and is calculated.

Calculate of the response utilizing Nernst equation.

Step 3 of three

The Nernst equation is as follows:

Calculate from as follows:

The and are as follows:

Within the response, cobalt undergoes oxidation and silver undergoes discount. The variety of electrons modified within the response is 2. Therefore, 2 is substituted for n and is calculated.

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The online cell response is .

The and are as follows:

The and are as follows:

The online cell response is .

The and are as follows:

The and are as follows:

0.0592V oxidation] [reduction] E E Е” cell n
AG
E ‘cell
AG=-nFE ‘cell
Co(s) Co 2+ (aq, 0.0155M)|| Ag’ (aq,3.50M)| Ag(s)
Anode: Co(s)->Co2 (aq)+2e Cathode: Ag (aq)+ e ->Ag(s)
Cо(3) > Со” (а)+ 2е 2Ag (a)+2 2Ag(s) Co(s)+2Ag’ (a)2 Ag (s)+Co (aq)
|Sn(s)+2Ag (a)->2 Ag(s)+Sn2′ (aq)
Е. cell
Со” (аq)+2е’ >Co(:) Ag’ (aq)+ е >Ag(s) -0.28 V +0.80 V
eell Eбоde – E aодe 0.80V-(0.28v) 1.08V
AG ГхТ
Е. cell
AG nFE, =-2molx96,485JV -molx1.08 V cell =-208407J =-208.4kJ
AG ГхТ
E ‘cell
0.0592Voxidation] discount] cell 1.08V-0.0592V log !0.0155M]| 2 3.50M] =1.15V
AG, ГхТ
E ‘cell
AG nFE, =-2molx96,485JV -molx1.15 V cеll =-221915J =-221.9kJ
AG, ГхТ
Co(s)+2Ag (aq)>2 Ag(s)+Co2 (aq)
Co(s)+2Ag (aq)>2 Ag(s)+Co2 (aq)
Co (s)+Co2 (a)2 Ag(s)+2Ag’ (aq)
Cо(:) + Ag” (ag) ->Ag(s)+Cо* (аg)
Co(s)+2Ag (a)2 Ag (s)+Co2″ (aq)
Е. cell
AG ГхТ
E° cell 1.08V AG 208.4kJ/mol
Е. cell
AG ГхТ
E° cell 1.08V AG 208.4kJ/mol
Е. cell
AG ГхТ
Е. AG 126.2kJ/mol =0.52V cell гхn

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