The voltage of a cell whose half cell reactions are given below is-Mg-2-2-e-rightarrow Mg-s-E-2-37V-Cu-2-2-e-rightarrow Cu-s- E-0-34V

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The voltage of a cell whose half cell reactions are given below is:
${M g}^{2 +} + 2 e^{-} \to M g (s); E = - 2.37 V$
${C u}^{2 +} + 2 e^{-} \to C u (s); E = + 0.34 V$

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The voltage of a cell whose half cell reactions are given below is

M g^{2 +} + 2 e^{-} \to M g (s)

;

E = - 2.37 V

(anode)

C u^{2 +} + 2 e^{-} \to C u (s)

E = + 0.34 V

(cathod)

View Solution

The voltage of a cell whose halfcells are given below is:

$M g^{2 +} + 2 e^{-} \to M g (s); E^{0} = - 2.37 V$

$C u^{2 +} + 2 e^{-} \to C u (s); E^{0} = + 0.34 V$ standard EMF of the cell is:

View Solution

A l^{3 +} (a q) + 3 e^{-} \to A l (s); E^{\circ} = - 1.66 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{\circ} = + 0.34 V

What voltage is produced under standard conditions to give a spontaneous reactions by combination of these two-half cells?

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If for the half-cell reactions

{C u}^{2 +} + e^{-} ⟶ C u^{+} E^{o} = 0.15 V

{C u}^{2 +} + 2 e^{-} ⟶ C u E^{o} = 0.34 V

Calculate

E^{o}

of the half cell reaction

{C u}^{+} + e^{-} ⟶ C u

Also predict whether

{C u}^{+}

undergoes disproportionation or not.

View Solution

If for the half cell reactions

C u^{2 +} + e^{-} \to C u^{+}

E^{o} = 0.15 V

C u^{2 +} + 2 e^{-} \to C u

E^{o} = 0.34 V

Calculate

E^{o}

of the half cell reaction

C u^{+} + e^{-} \to C u

also predict whether

C u^{+}

undergoes disproportionation or not.

View Solution