Chemical reactions involve interation of atoms and molecules. A large number of atoms `//` molecules `(` approximately `6.023xx10^(23))` are present in a few grams of any chemical compound varying with their atomic `//` molecular masses. To handle such large numbers conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry, biochemistry, electrochemistry, and radiochemistry. The following example illustrates a typical case, involving chemical `//` electrochemical reaction, which requires a clear understanding of the mole concept.
A `4.0M` aqueous solution of `NaCl` is prepared and `500mL` of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes `(` atomic mass of `Na ` is 23 and `Hg` is `200)(1F=96500C)`.
If the cathode is an `Hg` electrode, the maximum weight `(in g)` of amalgam formed from this solution is

Options

A. `200`
B. `225`
C. `400`
D. `446`

Answer

D

Explanation

`Na-Hg` (amalgam) formed `=2` moles at cathode.
`2` mole of amalgam `=23xx2+2xx200`
`=446`