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How many grams of  \mathrm{Cl_2}   gas are produced when molten \mathrm{\mathrm{NaCl}}  undergoes electrolysis at a current of\mathrm{ 3.24 \mathrm{~A}} for 30 minutes?

Option: 1

3.225 g


Option: 2

2.145 g


Option: 3

7.1 g


Option: 4

3.55 g


Answers (1)

best_answer

For electrolysis of molten NaCl, At Anode,
2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2+2 e^{-}
Means \mathrm{ 2 \mathrm{~F}}  charge is required to produce  \mathrm{ 71 \mathrm{gCl}_2}  gas.
Given Charge
\mathrm{ Q=I t } 
\mathrm{ Q=3.24 \times 30 \times 60 }
\mathrm{ Q=5832 \mathrm{C} }

\mathrm{ \because 2 \mathrm{~F} }  charge passed produce \mathrm{ \Rightarrow 1 \mathrm{~g} \mathrm{Cl}_2}
\mathrm{ \therefore 1 \mathrm{C}}   charge passed produce \mathrm{ \Rightarrow \frac{71}{2 \mathrm{~F}} \mathrm{~g} \mathrm{Cl}_2}
\mathrm{ \therefore 5832 \mathrm{C}}   charge passed produce
\mathrm{ \Rightarrow \frac{71}{2 \times 96500} \times 5832 }
\mathrm{ =2.145 \mathrm{~g} ~Cl_2 \text { gas } }.

Posted by

Ajit Kumar Dubey

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