Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential.   Pb2+(aq) + 2 e– → Pb(s) E° = –0.126 V   Fe3+(aq) + e– → Fe2+(s) E° = +0.771 V Choose the correct answer     a. Pb2+(aq) + Fe2+(s) → Pb(s) + Fe3+(aq); = +0.645 V b. Pb(s) + 2 Fe3+(aq) → Pb2+(aq) + 2 Fe2+(s); = +1.416 V c. Pb(s) + 2 Fe3+(aq) → Pb2+(aq) + 2 Fe2+(s); = +0.897 V d. Pb(s) + Fe3+(aq) → Pb2+(aq) + Fe2+(s); = +0.645 V e. Pb2+(aq) + 2 Fe2+(s) → Pb(s) + 2 Fe3+(aq); = +0.897 V

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Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential.

 

Pb2+(aq) + 2 e → Pb(s)

E° = –0.126 V

 

Fe3+(aq) + e → Fe2+(s)

E° = +0.771 V

Choose the correct answer

 
 

a. Pb2+(aq) + Fe2+(s) → Pb(s) + Fe3+(aq); = +0.645 V

b. Pb(s) + 2 Fe3+(aq) → Pb2+(aq) + 2 Fe2+(s); = +1.416 V

c. Pb(s) + 2 Fe3+(aq) → Pb2+(aq) + 2 Fe2+(s); = +0.897 V

d. Pb(s) + Fe3+(aq) → Pb2+(aq) + Fe2+(s); = +0.645 V

e. Pb2+(aq) + 2 Fe2+(s) → Pb(s) + 2 Fe3+(aq); = +0.897 V

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