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Zinc Ion

ntWhich one o...

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ntWhich one of the following metal do not evolve H2gas from dilute acidn nt(a) A (EO A+/A =0.25V)n nt(b) B (EO B/B+ = +0.22V)n nt(c) C (EOC+/C = -0.30V)n

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Q. Pairs of electrodes and their corresponding standard electrode potentials are given. Arrange the cells constructed by these electrodes in increasing order of emf values.

(a) E l e c t r o d e \to A, E^{o} = - 2.92 V

E l e c t r o d e \to B, E^{o} = - 2.71 V

(b) E l e c t r o d e \to C, E^{o} = - 0.760 V

E l e c t r o d e \to D, E^{o} = - 0.44 V

(c) E l e c t r o d e \to B, E^{o} = - 2.71 V

E l e c t r o d e \to D, E^{o} = - 0.44 V

(d) E l e c t r o d e \to A, E^{o} = - 2.92 V

E l e c t r o d e \to C, E^{o} = - 0.76 V

Given: $F e_{(s)} \to F e^{2 +} + 2 e^{-}; E^{o} = + 0.44 V$

$P b_{(s)} \to P b^{2 +} + 2 e^{-}; E^{o} = + 0.13 V$

$A g^{+} e^{-} \to A g; E^{o} = + 0.8 V$

$C u^{2 +} 2 e^{-} \to C u; E^{o} = + 0.34 V$

Which of the following metals will oxidise iron?

a) $A g$

b) $C u$

c) $P b$

d) None of these

Consider the following equation for a cell

A + B ⇌ C + D; E^{o} = X v o l t, K_{e q} = K_{1}

2 A + 2 B ⇌ 2 C + 2 D; E^{o} = y v o l t, K_{e q} = k_{2}

Q. Consider the following equations for a cell reaction :

A + B \to C + D; E^{o} = x v o l t, Δ G = Δ G_{1}

2 A + 2 B \to 2 C + 2 D; E^{o} = x v o l t, Δ G = Δ G_{2}

Deducted from the following

E^{o}

values of half cells, what combination of two half cells would result in a cell with the largest potential?

A^{3 -} \to A^{2 -} + e; E^{o} = 1.5 V

B^{2 +} + e \to B^{+}; E^{o} = 2.1 V

C^{2 +} + e \to C^{+}; E^{o} = + 0.5 V

D \to D^{2 +} + 2 e; E^{o} = - 1.5 V

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