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Standard VII

Chemistry

Faraday's Second Law

4.5 g of Alum...

Question

$4.5 g$ 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:

$44.8 L$

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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 D
$5.6 L$

No. Of equivalents of ' $A l$ ' deposited = $\left(\frac{4.5}{9}\right) = 0.5$
Volume of $H_{2}$ gas at STP = No. Of equivalents $\times$ Equivalent Volume= 0.5 $\times$ 11.2 = $5.6 L$

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Similar questions

Q. 4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from

A l^{3 +}

solution 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:

$4.5 g$ 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:

4.5 g

of aluminium (At. mass

= 27 a t m

) is deposited at cathode from

A l^{3 +}

solution 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___________.

4.5 g

of aluminum (at. mass 27amu) is deposited at cathode from

A l^{3 +}

solution 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

4.5

g of Aluminium(At mass

27

amu) is deposited at cathode form

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solution by a certain amount of electric charge. The volume of hydrogen produced at STP form

H^{+}

ions in solution by the same quantity of charge will be:

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4.5 g of Aluminium is deposited at cathode from Al3+ 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:

The correct option is D 5.6 L No. Of equivalents of 'Al' deposited = \(\left(\frac{4.5}{9}\right) = 0.5\) Volume of H2 gas at STP = No. Of equivalents × Equivalent Volume= 0.5× 11.2 = 5.6 L

$4.5 g$ 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:

The correct option is D
$5.6 L$

No. Of equivalents of ' $A l$ ' deposited = \(\left(\frac{4.5}{9}\right) = 0.5\)
Volume of $H_{2}$ gas at STP = No. Of equivalents $\times$ Equivalent Volume= 0.5 $\times$ 11.2 = $5.6 L$