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11 Dec 2019

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A voltaic cell is constructed from a standard Fe2+|Fe half cell (E°red = -0.440V) and a standard Al3+|Al half cell (E°red = -1.660V).

The anode reaction is:

______(aq)(s)(l)(g) + ______(aq)(s)(l)(g) -----> ______(aq)(s)(l)(g) + ______(aq)(s)(l)(g)



The cathode reaction is:

______(aq)(s)(l)(g) + ______(aq)(s)(l)(g) ------> ______(aq)(s)(l)(g) + ______(aq)(s)(l)(g)



The spontaneous cell reaction is:

________(aq)(s)(l)(g) + _______(aq)(s)(l)(g) ------> _______(aq)(s)(l)(g) + _______(aq)(s)(l)(g)



The cell voltage is _____V.

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13 Dec 2019

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Related questions

PLS only answer if you know what you're doing and if you are going to answer all of them, i got alot to do cuz of finals so i'd appreciate it if you answer them all correctly, thank you

1) Calculate the standard emf (electromotive force) for a voltaic cell whose cell reaction is represented by the balanced equation.

2H2O(l) → H2(g) + H2O2(aq)

2) Calculate the standard cell potential for a galvanic cell whose cell reaction is represented by the balanced equation.

2Fe(s) + 3I2(s) → 2Fe3+(aq) + 6I-(aq)

St. Red. Pot. (V)

Fe3+/Fe -0.04
I2/I- 0.54

3) For the voltaic cell shown, calculate the standard cell potential.

Pt(s) l H2O(l), H2O2(aq), H+(aq) ll H+(aq) l H2(g), Pt(s)

St. Red. Pot. (V)
H2O2/H2O 1.78
H+/H2

0

4)For the voltaic cell shown, calculate the standard cell potential.

Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)

St. Red. Pot. (V)

Mn2+/Mn -1.18
F2/F-

2.87

5)For the galvanic cell shown, calculate the Eo.

Fe(s) l Fe2+(aq) ll Cd2+(aq) l Cd(s)

St. Red. Pot. (V)

Fe2+/Fe -0.44
Cd2+/Cd -0.40

6) The value for the standard emf of a voltaic cell described by the cell notation is 1.88 V. Determine the value (V) of the standard half cell potential for the F2/F- couple.

Au(s) l AuCl4-(aq), Cl-(aq) ll F2(g) l F-(aq) l Pt(s)

St. Red. Pot. (V)

AuCl4-/Au 0.99
St. Red. Pot. (V)
H2O2/H2O 1.78
H+/H2 0

Which electrochemical reaction is spontaneous in a galvanic cell?

Ni2+(aq) + Cu(s) --> Ni(s) + Cu2+(aq)

Cr3+(aq) + Au(s) --> Cr(s) + Au3+(aq)

Cu2+(aq) + Co2+(aq) --> Cu+(aq) + Co3+(aq)

Cu2+(aq) + Sn(s) --> Cu(s) + Sn2+(aq)

Which electrochemical reaction is non-spontaneous in an electrolytic cell?

F2(g) + 2Cl-(aq) --> 2F-(aq) + Cl2(g)

Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)

Co2+(aq) + Pb(s) --> Co(s) + Pb2+(aq)

Mn2+(aq) + Ba(s) --> Mn(s) + Ba2+(aq)

Which electrochemical reaction is the most spontaneous, generating the highest cell voltage?

F2(g) + 2Cl-(aq) --> 2F-(aq) + Cl2(g)

Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)

Mn2+(aq) + Ba(s) --> Mn(s) + Ba2+(aq)

Cu2+(aq) + Sn(s) --> Cu(s) + Sn2+(aq)

Given the following notation for a galvanic cell diagram

Cd(s) │ Cd2+(aq) ║ Pb2+(aq) │ Pb(s)

Which one correctly represents the electrochemical reaction taking place in the galvanic cell?

Cd(s) + Pb2+(aq) --> Cd2+(aq) + Pb(s)

Cd2+(aq)+ Pb2+(aq) --> Cd(s)+ Pb(s)

Cd2+(aq) + Pb(s) --> Cd(s) + Pb2+(aq)

Cd2+(aq) + Pb2+(aq) --> Cd(s) + Pb2+(s)

Consider a Galvanic cell constructed from the following half cells, linked by a KCl salt bridge.

. an Al(s) electrode in 0.5 M Al2(SO4)3 solution

. a Pb(s) electrode in 1.0 M Pb(NO3)2 solution

Which electrode is the cathode?

Al

Pb

Al3+

Pb2+

1)Calculate forthe electrochemical cell below,

Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(aq) | Ag(s)

given the following standard reduction potentials.

Ag+(aq) + e- ->Ag(s) E° = +0.799 V

PbSO4(s)+ 2e- -> Pb(s) + SO4 2-(aq) E = -0.356 V

a) -1.954 V

b) -1.155 V

c) +0.443V

d) +1.155 V

2) Consider the following half- reactions:

Cu2+ (aq) + 2e- --> Cu(s)E = +0.34 V

Sn2+(aq) + 2e- --> Sn(s) E = -0.14 V

Fe2+(aq) +2e- --> Fe(s)E = -0.44 V

Al3+(aq) +3e- --> Al(s) E = -1.66 V

Mg2+(aq) + 2e---> Mg(s) E = -2.37 V

Which of the abovemetals or metal ions will reduce Fe2+ ?

a) Cu(s) andSn(s)

b) Cu2+(aq) andSn2+(aq)

c) Al3+(aq) andMg2+ (aq)

d) Al(s) andMg(s)

e) Sn(s) and Al3+(aq)

3) The following reaction occurs spontaneously

2H+ (aq) +Ca(s) --> Ca2+(aq) + H2(g)

Write a balanced recuction half-reaction-

a) 2H+(aq) + 2e --> H2(g)

b) 2H+ (aq) --> H2(g) + 2e-

c) H2(g) --> 2H+(aq) + 2e-

d) Ca(s) + 2e- --> Ca2+(aq)

e) Ca(s) --> Ca2+(aq) + 2e-

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