University College - Chemistry Chem 112A Lecture Notes - Lecture 27: Nernst Equation, Weighted Arithmetic Mean

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harlequinimpala978

13 Dec 2016

School

WUSTL

Department

University College - Chemistry

Course

University College - Chemistry Chem 112A

Professor

Bleeke John

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Document Summary

Cu2+ + e- cu+, (cid:3032)(cid:3031)(cid:2868) = 0. 16 v: 2. Cu+ + e- cu(s), (cid:3032)(cid:3031)(cid:2868) = 0. 52 v the g of each, adding since it is a state function, then getting a final (cid:3032)(cid:3031)(cid:2868) ) Doing this, we get (cid:3032)(cid:3031)(cid:2868) = 0. 34: you cannot ever calculate a new (cid:3032)(cid:3031)(cid:2868) by adding 2 (cid:3032)(cid:3031)(cid:2868) or 2 (cid:3042)(cid:2868, for g = g0 + rtlnq = -nf (cid:2868, = (cid:2868) (cid:3041)ln (cid:4666)(cid:4667, = (cid:2868) (cid:3041)ln(cid:4666)(cid:4667)= (cid:2868) (cid:2868). (cid:2868)(cid:2870)57(cid:3041) Where f = 96. 5 kcoul/mol ln(cid:4666)(cid:4667)= (cid:2868) (cid:2868). (cid:2868)59(cid:2870)(cid:3041) (cid:2869)(cid:2868)(cid:4666)(cid:4667)

Related Questions

Use the table of standard reduction potentials to complete the following table. Example is provided:

Electrodes	Half-reactions	E^o	E^o cell
Zn Cu	Zn(s) ---> Zn²⁺ +2e^- Cu²⁺+2e^- ---> Cu (s)	+0.76 V +0.34	+1.10 V
Cu Mg
Cu Fe
Zn Mg
Fe Mg
Zn Fe
Cu Cu

Any explanation/help would be appreciated!

write the oxidation half reactions corresponding to the reversereactions for the following reduction half reactions, and writetheir standard oxidation potentials.

a.) Zn^2+ (aq) + 2e^- -------> Zn (s) E^o = -0.76

b.) Cu^+(aq) + e^- ----------> Cu (s) E^o=0.52

c.) 2 I^- (aq) ---------> I2 (s) +2e^- E^o = 0.54

please explain if possible as well as the answers. For part C,it may not be the correct reduction half reaction of I2 (aq), so ifthe equation seems incorrect please let me know. I may have did itwrong.

Standard reduction potentials

Reduction half-reaction	E∘ (V)
Ag⁺(aq)+e⁻→Ag(s)	0.80
Cu²⁺(aq)+2e⁻→Cu(s)	0.34
Sn⁴⁺(aq)+4e⁻→Sn(s)	0.15
2H⁺(aq)+2e⁻→H₂(g)	0
Ni²⁺(aq)+2e⁻→Ni(s)	−0.26
Fe²⁺(aq)+2e⁻→Fe(s)	−0.45
Zn²⁺(aq)+2e⁻→Zn(s)	−0.76
Al³⁺(aq)+3e⁻→Al(s)	−1.66
Mg²⁺(aq)+2e⁻→Mg(s)	−2.37

Part A

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ^∘C) for the following reaction:

Express your answer numerically.

Part B

Calculate the standard cell potential (E^∘) for the reaction

if K = 3.04×10⁻³.

Express your answer to three significant figures and include the appropriate units.

lemongnat815

University College - Chemistry Chem 112A Lecture Notes - Lecture 27: Nernst Equation, Weighted Arithmetic Mean

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