Calculate the standard reduction potential of galvanic cell in which reaction are as follow Fe** (aq) + Ag+ (aq)- >Fe ++ (aq) + Ag(s) +++ += 0.77 volt, E° Agt/Ag = 0.80 Volt

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Calculate the standard cell potentials of galvanic cell in which the following reactions take place :

(Given $$ E_{OP}^{\circ} Cr , Cd , Fe^{2+} , Ag $$ are $$ 0.74\,V , 0.40\,V , -0.77\,V $$ and $$ -0.80\,V $$ respectively )

(a) $$\displaystyle 2Cr(s) + 3Cd^{2+}(aq.) \rightarrow 2Cr^{3+}(aq.) + 3Cd $$
(b) $$\displaystyle Fe^{2+} + Ag^{+}(aq) \rightarrow Fe^{3+}(aq.) + Ag(s) $$

Calculate the $$ \Delta_{r} G^{\circ} $$ and equilibrium constant of the reactions .

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Calculate the standard cell potential in (V) of the cell in which following reaction takes place:
$$Fe^{2+}(aq) + Ag^+(aq) \rightarrow Fe^{3+}(aq) + Ag(s)$$

Given that
$$E^o_{Ag^+/Ag} = xV$$
$$E^o_{Fe^{2+}/Fe} = yV$$
$$E^o_{Fe^{3+}/Fe} = zV$$

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Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
(i)

2 C r (s) + 3 C d^{2 +} (a q) \to 2 C r^{3 +} (a q) + 3 C d

(ii)

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

Calculate the

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and equilibrium constant of the reactions

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The standard electrode potential for the reactions,

A g^{+} (a q) + e^{-} \to A g (s)

S n^{2 +} (a q) + 2 e^{-} \to S n (s)

25^{\circ} C

are

0.80

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S n ∣ S n^{2 +} (1 M) ∣∣ A g^{+} (1 M) | A g

is :

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

Given standard electrode potentials

E_{F e^{3 +} / F e^{2 +}}^{\circ} = + 0.77 V and E_{A g^{+} / A g (s)}^{\circ} = + 0.80 V

If the reaction is feasible, enter

1.00

as answer elsewise enter

0.00

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