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Electrochemical Cells, Galvanic Cells

. Calculate E...

Question

. Calculate E°cell and ∆rG° for the following reaction at 25°C. A2+(aq) + B+(aq) → A3+(aq) + B(s) [Given KC = 1010, 1F = 96500 C, R = 8.314 JK–1 mol–1]

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Q. Calculate the equilibrium constant for the following reaction:

C u (s) + 2 {A g}^{+} (a q .) ⇌ {C u}^{2 +} (a q) + 2 A g (s)

25^{o} C

E_{c e l l}^{o} = 0.47 v o l t, R = 8.314 J K^{- 1} {m o l}^{- 1}, F = 96500 c o u l o m b

Q. Calculate the equilibrium constant for the reaction, at

25^{o} C

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

E_{c e l l}^{o} = 0.47 V, R = 8.134 J K^{- 1} F = 96500 C

Q. (a) The cell in which the following reaction occurs:

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

at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C

m o l^{- 1}

)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C

m o l^{- 1}

)

Q. a) Draw labelled diagram of Standard Hydrogen Electrode ( SHE ).
Write its half cell reaction of

E^{o}

value.
b) Calculate

△ r G^{⊝}

for the following reaction :

F e_{(a q)}^{+ 2} + A g_{(a q)}^{+} \to {F e}_{(a q)}^{+ 3} + A g_{(s)}

E_{C e l l}^{0} = + 0.03 V, F = 96500 C

Q. (a) The cell in which the following reaction occurs:

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

at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C

m o l^{- 1}

)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C

m o l^{- 1}

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