Two moles of electrons can do which of the following:
I. Reduce one mole of $A g^{+}$ to $A g$
II. Reduce one mole of $C u^{2 +}$ to $C u$
III. Reduce $\frac{2}{3}$ mole of $A l^{3 +}$ to $A l$

Question

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Answer 1

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

1 mole of $C u^{2 +}$ requires 2 moles of electrons to reduce to $C u$

$\frac{2}{3} A l^{3 +} + 2 e \to \frac{2}{3} A l$

$\frac{2}{3}$ moles of $A l^{3 +}$ requires 2 moles of electrons to reduce to $A l$ .

Hence, option $C$ is correct.

Answer 2

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

1 mole of

C u^{2 +}

requires 2 moles of electrons to reduce to

C u

\frac{2}{3} A l^{3 +} + 2 e \to \frac{2}{3} A l

\frac{2}{3}

moles of

A l^{3 +}

requires 2 moles of electrons to reduce to

A l

.

Hence, option

C

is correct.

Two moles of electrons can do which of the following:
I. Reduce one mole of $A g^{+}$ to $A g$
II. Reduce one mole of $C u^{2 +}$ to $C u$
III. Reduce $\frac{2}{3}$ mole of $A l^{3 +}$ to $A l$

$I, I I, a n d I I I$

$I a n d I I o n l y$

$I I a n d I I I o n l y$

$I o n l y$

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

1 mole of $C u^{2 +}$ requires 2 moles of electrons to reduce to $C u$

$\frac{2}{3} A l^{3 +} + 2 e \to \frac{2}{3} A l$

$\frac{2}{3}$ moles of $A l^{3 +}$ requires 2 moles of electrons to reduce to $A l$ .

Hence, option $C$ is correct.

One mole of electron passes through each of the solution of $A g N O_{3}, C u S O_{4}$ and $A l C l_{3}$ then $A g, C u$ and $A l$ are deposited at cathode. The molar ratio of $A g, C u$ and $A l$ deposited are:

The number of Faradays required to reduce one mole of $C u^{2 +}$ to metallic copper is:

How many coulombs are require for the following reductions?
(i) $1 m o l e$ of $A g^{+}$ ions to $A g$
(ii) $1 m o l e$ of $C u^{2 +}$ ions to $C u$
(iii) $1 m o l e$ of $M n O_{4}^{-}$ ions to $M n O_{4}^{2 -}$ .

How many faradays are needed to reduce $2$ gram-mole of $C u^{2 +}$ to $C u$ metal?

How much charge is required for the reduction of :
(a) 1 mole of $A l^{3 +}$ to $A l$
(b) 1 mole of $C u^{2 +}$ to $C u$
(c) 1 mole of $M n O_{4}^{-}$ to $M n^{2 +}$
(d) 1 mole of $C r_{2} O_{7}^{2 -}$ to $C r^{3 +}$

Revise with Concepts

Electrolytic Cells and Electrolysis

Faraday's Law

Products of Electrolysis

Two moles of electrons can do which of the following: I. Reduce one mole of Ag+ to Ag II. Reduce one mole of Cu2+ to Cu III. Reduce 32​ mole of Al3+ to Al

I,II, and III

I and II only

II and III only

I only

Cu2++2e→Cu 1 mole of Cu2+ requires 2 moles of electrons to reduce to Cu 32​Al3++2e→32​Al 32​ moles of Al3+ requires 2 moles of electrons to reduce to Al. Hence, option C is correct.

One mole of electron passes through each of the solution of AgNO3​,CuSO4​ and AlCl3​ then Ag, Cu and Al are deposited at cathode. The molar ratio of Ag, Cu and Al deposited are:

The number of Faradays required to reduce one mole of Cu2+ to metallic copper is:

How many coulombs are require for the following reductions? (i) 1 mole of Ag+ ions to Ag (ii) 1 mole of Cu2+ ions to Cu (iii) 1 mole of MnO4−​ ions to MnO42−​.

How many faradays are needed to reduce 2 gram-mole of Cu2+ to Cu metal?

How much charge is required for the reduction of : (a) 1 mole of Al3+ to Al (b) 1 mole of Cu2+ to Cu (c) 1 mole of MnO4−​ to Mn2+ (d) 1 mole of Cr2​O72−​ to Cr3+

Revise with Concepts

Electrolytic Cells and Electrolysis

Faraday's Law

Products of Electrolysis

Two moles of electrons can do which of the following:
I. Reduce one mole of $A g^{+}$ to $A g$
II. Reduce one mole of $C u^{2 +}$ to $C u$
III. Reduce $\frac{2}{3}$ mole of $A l^{3 +}$ to $A l$

$I, I I, a n d I I I$

$I a n d I I o n l y$

$I I a n d I I I o n l y$

$I o n l y$

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

1 mole of $C u^{2 +}$ requires 2 moles of electrons to reduce to $C u$

$\frac{2}{3} A l^{3 +} + 2 e \to \frac{2}{3} A l$

$\frac{2}{3}$ moles of $A l^{3 +}$ requires 2 moles of electrons to reduce to $A l$ .

Hence, option $C$ is correct.

One mole of electron passes through each of the solution of $A g N O_{3}, C u S O_{4}$ and $A l C l_{3}$ then $A g, C u$ and $A l$ are deposited at cathode. The molar ratio of $A g, C u$ and $A l$ deposited are:

The number of Faradays required to reduce one mole of $C u^{2 +}$ to metallic copper is:

How many coulombs are require for the following reductions?
(i) $1 m o l e$ of $A g^{+}$ ions to $A g$
(ii) $1 m o l e$ of $C u^{2 +}$ ions to $C u$
(iii) $1 m o l e$ of $M n O_{4}^{-}$ ions to $M n O_{4}^{2 -}$ .

How many faradays are needed to reduce $2$ gram-mole of $C u^{2 +}$ to $C u$ metal?

How much charge is required for the reduction of :
(a) 1 mole of $A l^{3 +}$ to $A l$
(b) 1 mole of $C u^{2 +}$ to $C u$
(c) 1 mole of $M n O_{4}^{-}$ to $M n^{2 +}$
(d) 1 mole of $C r_{2} O_{7}^{2 -}$ to $C r^{3 +}$