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The standard cell potential (Eecell) for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [ Zn2+] = 1.0 M and [Pb2+] = 2.0 X 10e-4 M.

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AP Chemistry
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Solve problems involving cell potentials under nonstandard conditions
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Related questions

Consider the following table of standard reduction potentials.

Half-reaction E o (V)
Cu2+(aq) + 2e? ? Cu(s) +0.34
Pb2+(aq) + 2e? ? Pb(s) -0.126
Cd2+(aq) + 2e? ? Cd(s) -0.403
Zn2+(aq) + 2e? ? Zn(s) -0.76


Based on these values, which of the following choices represents the correct combination of cell reaction and standard cell potential?

Cu2+(aq) + Cd(s) ? Cu(s) + Cd2+(aq), +0.06 V
Cu2+(aq) + Zn(s) ? Cu(s) + Zn2+(aq), ?0.42 V
Pb2+(aq) + Cd(s) ? Pb(s) + Cd2+(aq), +0.53 V
Pb2+(aq) + Zn(s) ? Pb(s) + Zn2+(aq), +0.63 V

the standard cell potential for the reaction below is =0.63 V. thecell potential under non standard conditions for this reaction is___ V. when (Zn^2 + )= 1.0 M and (Pb^2)=2.0x 10^-4 M.
Pb^2 (aq) + Zn (s)------>Zn^2 (aq)= Pb(s)

The standard cell potential of the reaction below is E°cell = 0,76 V.

When P = 1,0 atm and [Zn2+] = 1,0 M the cell potential is Ecell = 0,66 V. H2 What is [H+] at that point?

Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g)

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