Using the following standard reduction potentials Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq)...
Using the following standard reduction potentials
| Fe3+(aq) + e- → Fe2+(aq) | E° = +0.77 V |
| Pb2+(aq) + 2 e- → Pb(s) | E° = -0.13 V |
calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.
Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s)
Group of answer choices
E° = -0.90 V, spontaneous
E° = -0.90 V, nonspontaneous
E° = +0.90 V, nonspontaneous
E° = +0.90 V, spontaneous
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Using the following standard reduction potentials
Fe3+(aq) + e- → Fe2+(aq)
E° = +0.77 V
Pb2+(aq)...
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E⁰red
= −0.126 V
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E⁰red
= +1.358 V
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Cl−(aq)?
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Cl−(aq)?
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Pb(s)
E⁰red
= −0.126 V
Cl2(g) + 2 e− → 2
Cl−(aq)
E⁰red
= +1.358 V
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Cl−(aq)?
Pb(s) ; or Cl−(aq)
(b) Which is the most difficult to oxidize, Pb(s) or
Cl−(aq)?
Pb(s); or Cl−(aq)
(c) Is Pb(s) able to reduce Cl2(g) in
a spontaneous reaction?
is able; or is not able
(d) Is Cl−(aq)
able to reduce Pb2+(aq)...
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