The - G - for the Daniell Cell has been found to be -212-3 kJ at 25- C- Calculate the equilibrium constant for the cell reaction- A- 4-61 - 1037B- 1-64 - 1037C- 8-98 - 1025D- 9-05 - 1027

The correct option is B Δ G^∘= 2.303RTlogK_c ⇒ logK_c=Δ G^∘/ 2.303RT = 212300/ 2.303 × 8.314 × 298 ⇒ log K_c=37.20 ⇒ K_c=Antilog(37.20) ⇒ K_c=1.64 × 10^37 ...

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Byju's Answer

Standard VII

Chemistry

Equilibrium Constant from Nernst Equation

The Δ G ∘ for...

Question

The $Δ G^{\circ}$ for the Daniell Cell has been found to be - 212.3 kJ at $25^{\circ} C$ . Calculate the equilibrium constant for the cell reaction.

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Solution

The correct option is B
$Δ G^{\circ} = - 2.303 R T l o g K_{c} \Rightarrow l o g K_{c} = \frac{Δ G^{\circ}}{- 2.303 R T} = \frac{- 212300}{- 2.303 \times 8.314 \times 298} \Rightarrow l o g K_{c} = 37.20 \Rightarrow K_{c} = A n t i l o g (37.20) \Rightarrow K_{c} = 1.64 \times 10^{37}$

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