The electrical work done during the reaction at 298 K-2Hgl - Cl2g- Hg2Cl2s- isGiven that E-Cl2-Cl- - 1-36 V- E-Hg2Cl2-Hg-Cl- 0-27V - PCl2 - 1 atm-

Δ G^∘ = electrical work done = n F E^∘_cell = 2 × 96500 × (1.36 0.27)J = 210.37 kJ ...

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

Byju's Answer

Standard XI

Chemistry

Gibb's Energy and Nernst Equation

The electrica...

Question

The electrical work done during the reaction at 298 K:
$2 H g_{(l)} + C l_{2 (g)} \to H g_{2} C l_{2 (s)}, i s G i v e n t h a t E_{\frac{C l_{2}}{C l^{-}}}^{\circ} = 1.36 V; E_{\frac{H g_{2} C l_{2}}{H g, C l^{-}}}^{\circ} = 0.27 V; P_{C l_{2}} = 1 a t m,$

$210.37 k J m o l^{- 1}$

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

$105.185 k J m o l^{- 1}$

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

$420.74 k J m o l^{- 1}$

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

$110.37 k J m o l^{- 1}$

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

Open in App

Solution

The correct option is A
$210.37 k J m o l^{- 1}$

$- Δ G^{\circ} =$ electrical work done $= n F E_{c e l l}^{\circ} = 2 \times 96500 \times (1.36 - 0.27) J = 210.37 k J$

Suggest Corrections

Similar questions

The electrical work done during the reaction at 298 K:
$2 H g_{(l)} + C l_{2 (g)} \to H g_{2} C l_{2 (s)}, i s G i v e n t h a t E_{\frac{C l_{2}}{C l^{-}}}^{\circ} = 1.36 V; E_{\frac{H g_{2} C l_{2}}{H g, C l^{-}}}^{\circ} = 0.27 V; P_{C l_{2}} = 1 a t m,$

Calculate the useful work done during the reaction in kJ/mol.
$A g (S) + \frac{1}{2} C l_{2} (g) \to A g C l (s)$
Given that $E_{C l_{2} / {C l}^{-}}^{0} = + 1.36 V$
and $E_{A g^{+} | A g C l | C l^{-}}^{0} = + 0.220 V$
$P_{C l_{2}} = 1 atm$ and T = 298 K