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Two standard reduction potentials are given below. Pb2+(aq) + 2 e− → Pb(s)     E⁰red  = −0.126...

Two standard reduction potentials are given below.

Pb2+(aq) + 2 e− → Pb(s)    

E⁰red 

= −0.126 V
Cl2(g) + 2 e− → 2 Cl−(aq)    

E⁰red 

= +1.358 V

(a) Which is a stronger reducing agent, Pb(s) or 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) in a spontaneous reaction?

is able; or is not able    

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Stren red o rcutt to oxidize 14 -) 2+ -1 es Spon tan toud Rcactrz Pb Ni SPOntan tous

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