(b) Given the overall equation a redox reaction alongside the standard reduction potentials, E |A(s) + B³*(aq) = A*(aq) + B²* (aq)| A* (aq) + e¯ = A(s) E° = +0.799 V B*(aq) + e¯ = B²*(aq) E° = +0.771 V i. Calculate AG°. Determine whether the reaction is spontaneous. Show your working clearly. (F = 96500 Coulomb/equivalent) ii. Calculate the equilibrium constant K for the reaction at 40 °C.

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(b) Given the overall equation a redox reaction alongside the standard reduction potentials,
E°:
| A(s) + B³* (aq) = A* (aq) + B²*(e
A* (aq) + e-= A(s)
B* (aq) + e= B2+*(aq)
E° = +0.799 V
E° = +0.771 V
i. Calculate AG". Determine whether the reaction is spontaneous. Show your working
clearly. (F = 96500 Coulomb/equivalent)
ii. Calculate the equilibrium constant K for the reaction at 40 °C.
Transcribed Image Text:(b) Given the overall equation a redox reaction alongside the standard reduction potentials, E°: | A(s) + B³* (aq) = A* (aq) + B²*(e A* (aq) + e-= A(s) B* (aq) + e= B2+*(aq) E° = +0.799 V E° = +0.771 V i. Calculate AG". Determine whether the reaction is spontaneous. Show your working clearly. (F = 96500 Coulomb/equivalent) ii. Calculate the equilibrium constant K for the reaction at 40 °C.
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