MHT CET · Chemistry · Electrochemistry
Calculate the quantity of electricity required to liberate 0.1 mole of chlorine gas during electrolysis of molten sodium chloride.
- A 9665 C
- B 19300 C
- C 14500 C
- D 96500 C
Answer & Solution
Correct Answer
(B) 19300 C
Step-by-step Solution
Detailed explanation
During electrolysis of molten NaCl , the following reaction takes place at anode:
\(2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2+2 \mathrm{e}^{-}\)
1 mole of \(\mathrm{Cl}_2\) is liberated with 2 moles of electrons.
\(\therefore 0.1 \text { mole of } \mathrm{Cl}_2 \text { will be liberated with }\)\(0.2 \text { moles}\)\(\text { of electrons.}\)
\(2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2+2 \mathrm{e}^{-}\)
1 mole of \(\mathrm{Cl}_2\) is liberated with 2 moles of electrons.
\(\therefore 0.1 \text { mole of } \mathrm{Cl}_2 \text { will be liberated with }\)\(0.2 \text { moles}\)\(\text { of electrons.}\)
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