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Standard XII

Chemistry

Faraday's Second Law

A quantity of...

Question

A quantity of electrical charge that brings about the deposition of 4.5 g $A l$ from $A l^{3 +}$ at the cathode will also produce the following volume (STP) of $H_{2} (g)$ from $H^{\oplus}$ at the cathode:

44.8 L

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22.4 L

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11.2 L

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5.6 L

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Solution

The correct option is C $5.6 L$
$2 H^{\oplus} + 2 e^{-} \to H_{2}$
$A l^{3 +} + 3 e^{-} \to A l$
$\frac{W (H_{2})}{W (A l)} = \frac{E q (H_{2})}{E q (A l)} = \frac{1}{9}$
$W (H_{2}) = 4.5 \times \frac{1}{9} = 0.5 g = \frac{1}{4} m o l H_{2}$
$= 5.6 L H_{2} a t S T P$

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$4.5 g$ of Aluminium is deposited at cathode from $A l^{3 +}$ solutions by a certain quantity of electric charge. The volume of hydrogen produced at STP from $H^{+}$ ions in solution by the same quantity of electric charge will be:

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A quantity of electrical charge that brings about the deposition of 4.5 g Al from Al3+ at the cathode will also produce the following volume (STP) of H2(g) from H⊕ at the cathode:

The correct option is C 5.6L2H⊕+2e−→H2Al3++3e−→AlW(H2)W(Al)=Eq(H2)Eq(Al)=19W(H2)=4.5×19=0.5g=14molH2=5.6LH2atSTP

A quantity of electrical charge that brings about the deposition of 4.5 g $A l$ from $A l^{3 +}$ at the cathode will also produce the following volume (STP) of $H_{2} (g)$ from $H^{\oplus}$ at the cathode:

The correct option is C $5.6 L$
$2 H^{\oplus} + 2 e^{-} \to H_{2}$
$A l^{3 +} + 3 e^{-} \to A l$
$\frac{W (H_{2})}{W (A l)} = \frac{E q (H_{2})}{E q (A l)} = \frac{1}{9}$
$W (H_{2}) = 4.5 \times \frac{1}{9} = 0.5 g = \frac{1}{4} m o l H_{2}$
$= 5.6 L H_{2} a t S T P$