Half cell reactions for some electrodes are given below-A -e- - A- E-0-96V-B- -e- - B- E-0-12V-C- -e- - C E-0-18V-D- -e- - D E-1-12V-Construct a cell which can produce largest potential-

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Standard XII

Chemistry

EMF

Half cell rea...

Question

Half cell reactions for some electrodes are given below A +e- --> A+ E⁰=0.96V B- +e- --> B²- E⁰=-0.12V C+ +e- --> C E⁰=+0.18V D²+ +e- --> D E⁰=-1.12V Construct a cell which can produce largest potential

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Half cell reactions for some electrodes are given below:

A + e^{-} ⟶ A^{-}; E^{0} = 0.96 V

II.

B^{-} + e^{-} ⟶ B^{2 -}; E^{o} = - 0.12 V

III.

C^{+} + e^{-} ⟶ C; E^{o} = + 0.18 V

IV.

D^{2 +} + {2 e}^{-} ⟶ D; E^{o} = - 1.12 V

The largest potential will be generated in which cell?

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) Electrode

\to A, E^{\circ} =

- 2.92

V and Electrode

\to B, E^{\circ} =

- 2.71

V
(b) Electrode

\to C, E^{\circ} =

- 0.760

V and Electrode

\to D, E^{\circ} =

- 0.44

V
(c) Electrode

\to B, E^{\circ} =

- 2.71

V and Electrode

\to D, E^{\circ} =

- 0.44

V
(d) Electrode

\to A, E^{\circ} =

- 2.92

V and Electrode

\to C, E^{\circ} =

0.76

Deduced from the following $E^{\circ}$ values of half cells, what combination of two half cells would result in a cell with the largest potential?
(i) $A^{3 -} \to A^{2 -} + e; E^{\circ} = 1.5 V$ (ii) $B^{2 +} + e \to B^{+}; E^{\circ} = 2.1 V$
(iii) $C^{2 +} + e \to C^{+}; E^{\circ} = + 0.5 V$ (iv) $D \to D^{2 +} + 2 e; E^{\circ} = - 1.5 V$

Q. Given the following half-cell reactions and corresponding reduction potentials:

S NO	Reaction	$E^{0}$ in volts
I	$A + e^{-} ⟶ A^{-}$	$- 0.24 V$
II	$B + 2 e^{-} ⟶ B^{2 -}$	$+ 1.25 V$
III	$C + 3 e^{-} ⟶ C^{3 -}$	$- 0.25 V$
IV	$D + 2 e^{-} ⟶ D^{2 -}$	$+ 0.68 V$
V	$E + 4 e^{-} ⟶ E^{4 -}$	$- 0.38 V$