Calculate E.M.F. of following cell at 298 K Zn(s) | ZnSO4(0.01 M)||CuSO4( 1.0 M ) |Cu (s) if E° cell = 2.0 V

Question

Calculate E.M.F. of following cell at 298 K Zn(s) | ZnSO4(0.01 M)||CuSO4( 1.0 M ) |Cu (s) if E° cell = 2.0 V (A) 2.0 V (B) 2.0592 V (C) 2.0296 (D) 1.0508 V

Tardigrade Admin · Accepted Answer

Key Idea General form of Nernst equation is

E_{(M^{n +} / M)} = E_{(M^{n +} / M)}^{0} - \frac{RT}{n F} ln \frac{[ M ]}{[ M ^{n +} ]}

Oxidation

Z n (s) ⟶ Z n^{2 +} (a q) [0.01 M] + 2 e^{-}

Reduction

C u^{2 +} (a q) [1.0] M ⟶ C u (s)

Using Nernst equation,

E_{cell} = E_{cell}^{\circ} - \frac{0.059}{2} lo g [\frac{1}{100}]

= 2 - \frac{0.59}{2} \times - 2 = 2 + 0.059

= 2.059 V

Q. Calculate $E$ . $M$ . $F$ . of following cell at $298 K$ $Z n (s) ∣ Z n S O_{4} (0.01 M) ∣∣ C u S O_{4} (1.0 M) ∣ C u (s)$ if $E^{\circ}$ cell $= 2.0 V$

$2.0 V$

$2.0592 V$

$2.0296$

$1.0508 V$

Q. Calculate E.M.F. of following cell at 298K Zn(s)∣ZnSO4​(0.01M)∣∣CuSO4​(1.0M)∣Cu(s) if E∘ cell =2.0V

2.0V

2.0592V

2.0296

1.0508V

Key Idea General form of Nernst equation is E(Mn+/M)​=E(Mn+/M)0​−nFRT​ln[Mn+][M]​ Oxidation Zn(s)⟶Zn2+(aq)[0.01M]+2e− Reduction Cu2+(aq)[1.0]M⟶Cu(s) Using Nernst equation, Ecell ​=Ecell ∘​−20.059​log[1001​] =2−20.59​×−2=2+0.059 =2.059V

Q. Calculate $E$ . $M$ . $F$ . of following cell at $298 K$ $Z n (s) ∣ Z n S O_{4} (0.01 M) ∣∣ C u S O_{4} (1.0 M) ∣ C u (s)$ if $E^{\circ}$ cell $= 2.0 V$

$2.0 V$

$2.0592 V$

$2.0296$

$1.0508 V$