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Question

An electric current of $$100$$ ampere is passed through a molten liquid of sodium chloride for $$5$$ hours.  Calculate the volume of chlorine gas liberated at the electrode at $$NTP$$.


Solution

The reaction taking place at anode is :
$$2Cl^{-} \rightarrow Cl_2 + 2e^{-}$$
Q=I*t = 100*5*60*60 coulumb
The amount of chlorine liberated by passing 100*5*60*60 coulumb of electric charge =$$\dfrac{1}{2*96500}$$*100*5*60*60 = 9.3264 mole
Volume of $$Cl_2$$ liberated at NTP = 9.3264*22.4 = 208.91L.

Chemistry

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