`Ag^(+)(aq) + e^(-) rightarrow Ag(s)` `E^(@) = 0.80V` `Co^(2+)(aq) + 2e(-) rightarrow Co(s)` `E^(@) = -0.28V` Use the standard reduction potentials to determine the standard potential for the reaction: `Co(s) + 2Ag^(+)(aq_) rightarrow Co^(2+)(aq) + 2Ag(s)`A. 0.52VB. 0.66VC. 1.08VD. 1.88V

`Ag^(+)(aq) + e^(-) rightarrow Ag(s)` `E^(@) = 0.80V` `Co^(2+)(aq) + 2

1.	`Ag^(+)(aq) + e^(-) rightarrow Ag(s)` `E^(@) = 0.80V` `Co^(2+)(aq) + 2e(-) rightarrow Co(s)` `E^(@) = -0.28V` Use the standard reduction potentials to determine the standard potential for the reaction: `Co(s) + 2Ag^(+)(aq_) rightarrow Co^(2+)(aq) + 2Ag(s)`A. 0.52VB. 0.66VC. 1.08VD. 1.88V
Answer» Correct Answer - C

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`Ag^(+)(aq) + e^(-) rightarrow Ag(s)` `E^(@) = 0.80V` `Co^(2+)(aq) + 2e(-) rightarrow Co(s)` `E^(@) = -0.28V` Use the standard reduction potentials to determine the standard potential for the reaction: `Co(s) + 2Ag^(+)(aq_) rightarrow Co^(2+)(aq) + 2Ag(s)`A. 0.52VB. 0.66VC. 1.08VD. 1.88V

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