Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows:
Ag⁺(aq) + e^-? Ag(s)
E° = 0.8 V
Co²⁺(aq) +2 e^-? Co(s)
E° = -0.277 V

Question

Calculate the standard cell potential (

E _ { \text {cell } } ^ { \circ }

) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows:
Ag⁺(aq) + e^-? Ag(s)
E° = 0.8 V
Co²⁺(aq) +2 e^-? Co(s)
E° = -0.277 V

Quizplus · Accepted Answer

The standard cell potential is calculated using the formula:$E _ { \text {cell } } ^ { \circ }$ = $E _ { \text {red } } ^ { \circ }$ (cathode) - $E _ { \text {red } } ^ { \circ }$ (anode)In this case, the cathode is the reduction of Ag⁺ to Ag, and the anode is the oxidation of Co to Co²⁺. Therefore, the standard cell potential is:$E _ { \text {cell } } ^ { \circ }$ = 0.8 V - (-0.277 V) = 1.077 VTherefore, the correct answer is A.

Calculate the Standard Cell Potential Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​

Calculate the Standard Cell Potential $E _ { \text {cell } } ^ { \circ }$