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Question
When one Faraday current is passed, which of the following would deposit 1g atomic weight of the metal?
When one Faraday current is passed, which of the following would deposit 1g atomic weight of the metal?
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Solution
The correct option is A NaCl
Gram-atomic weight definition is the mass of one mole of an element equal in grams to the atomic weight
No. of gram equivalents = Weight of substance / Equivalent weight
Now, as the valency of Na+ in NaCl is 1,
Equivalent weight = Molar mass/ valency = Molar mass/ 1 = molar mass.
1 F will deposit only 1 mole (or one gram equivalent) of Na metal.
No. of equivalent weight deposited = molar mass / equivalent weight = 1 gm atomic weight.
Hence, option A is correct.
Gram-atomic weight definition is the mass of one mole of an element equal in grams to the atomic weight
No. of gram equivalents = Weight of substance / Equivalent weight
Now, as the valency of Na+ in NaCl is 1,
Equivalent weight = Molar mass/ valency = Molar mass/ 1 = molar mass.
1 F will deposit only 1 mole (or one gram equivalent) of Na metal.
No. of equivalent weight deposited = molar mass / equivalent weight = 1 gm atomic weight.
Now, as the valency of Na+ in NaCl is 1,
Equivalent weight = Molar mass/ valency = Molar mass/ 1 = molar mass.
1 F will deposit only 1 mole (or one gram equivalent) of Na metal.
No. of equivalent weight deposited = molar mass / equivalent weight = 1 gm atomic weight.
Hence, option A is correct.
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