Question

Chemical reactions involve interaction of atoms and molecules. A large number of atoms $/$ molecules (approximately $6.023 \times 10^{23}$ ) 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 $4.0$ 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 $=96,500$ coulombs). The total number of moles of chlorine gas evolved is

• A. 0.5
• B. 1.0
• C. 2.0
• D. 3.0

Answer 1

Answer: (B)

$NaCl \rightarrow Na ^{+}+ Cl ^{-}$
At the anode:
$2 Cl ^{-} \rightarrow Cl _{2}$
Moles of $Cl ^{-}=2$ in $500\, ml$.
Therefore, $1$ mole of $Cl _{2}$ is evolved.