You visited us 1 times! Enjoying our articles? Unlock Full Access!

Gibb's Energy and Nernst Equation

The value of ...

Question

The value of $Δ G (k J m o l^{- 1})$ for the given cell is (take $1 F = 96500 C m o l^{- 1})$ :

-5.7

No worries! We‘ve got your back. Try BYJU‘S free classes today!

5.7

No worries! We‘ve got your back. Try BYJU‘S free classes today!

11.4

No worries! We‘ve got your back. Try BYJU‘S free classes today!

-11.4

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D -11.4
$M | M^{2 +}$ (saturated solution of a sparingly soluble salt $M X_{2}) | | M^{2 +} 0.001 m o l d m^{- 3} | M$
Reactions of cell
At anode : $M (s) \to M^{2 +} (a q .) + 2 e^{-}$
At cathode : $M^{2 +} (a q .) + 2 e^{-} \to M (s)$
So no of reactions taking part in reaction is 2
Also, as we know
$Δ G = - n F E$
$Δ G = - n F E_{c e l l} = - 2 \times 96500 \times 0.059 = - 113873 k J / m o l$
$= - 11.387 k J / m o l = - 11.4 k J / m o l e$

Suggest Corrections

Similar questions

△ G (k J m o l^{- 1})

1 F = 96500 C m o l^{- 1})

M | M^{2 +}

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

M^{2 +}

Δ G (k J m o l^{- 1})

1 F = 96500 C m o l^{- 1})

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

E_{cell}^{⊝} = 0.236 V

m o l^{- 1}

m o l^{- 1}

△_{r} G^{0}

M g (s) + C u^{2 +} (a q) \to M g^{2 +} (a q) + C u (s)

E_{c e l l}^{0} = + 2.71 V, 1 F = 96500 C m o l^{- 1}

Δ_{r} G^{0}

M g (s) + {C u}^{2 +} (a q) \to {M g}^{2 +} (a q) + C u (s)

E_{c e l l}^{0} = 2.71 V, 1 F = 96500 C {m o l}^{- 1}

Join BYJU'S Learning Program