JEE MAIN - Chemistry (2020 - 9th January Morning Slot - No. 12)
108 g of silver (molar mass 108 g mol–1) is
deposited at cathode from AgNO3(aq) solution
by a certain quantity of electricity. The
volume (in L) of oxygen gas produced at
273 K and 1 bar pressure from water by the
same quantity of electricity is _______.
Answer
5.66to5.68
Explanation
Cathode : Ag+(aq) + e- $$ \to $$ Ag(s)
Moles of Ag deposited = $${{108} \over {108}}$$ = 1 mole
Anode : 2H2O $$ \to $$ O2 + 4H+ + 4e-
Here we have to find volume of O2 evolved.
Equivalance of Ag = Equivalance of O2
$$ \Rightarrow $$ 1 $$ \times $$ 1 = nO2 $$ \times $$ 4
$$ \Rightarrow $$ nO2 = $${1 \over 4}$$ mol
$$ \therefore $$ Volume of O2 evolved
= $${1 \over 4}$$ $$ \times $$ 22.4
= 5.6 lit
Moles of Ag deposited = $${{108} \over {108}}$$ = 1 mole
Anode : 2H2O $$ \to $$ O2 + 4H+ + 4e-
Here we have to find volume of O2 evolved.
Equivalance of Ag = Equivalance of O2
$$ \Rightarrow $$ 1 $$ \times $$ 1 = nO2 $$ \times $$ 4
$$ \Rightarrow $$ nO2 = $${1 \over 4}$$ mol
$$ \therefore $$ Volume of O2 evolved
= $${1 \over 4}$$ $$ \times $$ 22.4
= 5.6 lit
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