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General Chemistry

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Cell Voltage and Redox Half Reactions

CHEM-VM24YK

Given the standard cell potential is $0.47 \textrm { V}$ for the redox reaction below:

$${ { Cu }^{ 2+ } }_{ \left( aq \right) }+{ Pb }_{ \left( s \right) }\longrightarrow { Cu }_{ \left( s \right) }+{ { Pb }^{ 2+ } }_{ \left( aq \right) }$$

Calculate the potential for the reduction half reaction :

$${ { Cu }^{ 2+ } }_{ \left( aq \right) }+{ 2{ e }^{ - } }\longrightarrow { Cu }_{ \left( s \right) }$$

given:

$${ { Pb }^{ 2+ } }_{ \left( aq \right) }+{ 2{ e }^{ - } }\longrightarrow { Pb }_{ \left( s \right) } \qquad { E }^{ \circ }=-0.13\textrm{ V}$$