Question

Read the passage given below and answer the question:
Chemical reactions involve the interaction of atoms and molecules. A large number of atoms/molecules (approximately $6.023\times {10}^{23}$) are present in 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 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200; 1 faraday =96500 coulombs).
If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from this solution is:

• A. 200
• B. 225
• C. 400
• D. 446

Answer 1

The correct option is D 446

Moles of $N{a}^{+}$ ion $=2$ $moles$
So, maximum $2$ $moles$ of $Na-Hg$ amalgam will be formed.

Weight $=2\times (23+200)=446$ $gm$