Standard electrode potential of half-cell reactions are given below C u2++2 e- arrow C u ; E°=0.34 V Z n2++2 e- arrow Z n ; E°=-0.76 V What is the emf of the cell?

Question

Standard electrode potential of half-cell reactions are given below C u2++2 e- arrow C u ; E°=0.34 V Z n2++2 e- arrow Z n ; E°=-0.76 V What is the emf of the cell? (A) + 1.10 V (B) −1.10 V (C) −0.42 V (D) +0.42 V

Tardigrade Admin · Accepted Answer

Z n arrow Z n2++2 e-(oxidation half-reaction) C u2++2 e- arrow C u (reduction half-reaction) Emf of the cell = standard oxidation potential of zinc electrode + standard reduction potential of Cu electrode =0.76 V +0.34 V =1.10 V

Q. Standard electrode potential of half-cell reactions are given below
$C u^{2 +} + 2 e^{-} \to C u; E^{\circ} = 0.34 V$
$Z n^{2 +} + 2 e^{-} \to Z n; E^{\circ} = - 0.76 V$
What is the emf of the cell?

+ 1.10 V

−1.10 V

−0.42 V

+0.42 V

$Z n \to Z n^{2 +} + 2 e^{-}$ (oxidation half-reaction)
$C u^{2 +} + 2 e^{-} \to C u$ (reduction half-reaction)
Emf of the cell $=$ standard oxidation potential of zinc
electrode $+$ standard reduction potential of Cu electrode
$= 0.76 V + 0.34 V = 1.10 V$

Q. Standard electrode potential of half-cell reactions are given below Cu2++2e−→Cu;E∘=0.34V Zn2++2e−→Zn;E∘=−0.76V What is the emf of the cell?