9.65 ampere of current was passed for one hour through Daniel cell. The loss of mass of zinc anode is :
A
11.76g
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B
1.176g
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C
5.88g
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D
2.94g
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Solution
The correct option is A 11.76g The quantity of electricity passed =Q(C)=I(A)×t(s)=9.65A×3600s=34740C. Molar mass of zinc = 65.4 gmol Moles of electrons passed =Q(C)96500Cmole−=34740C96500Cmole−=3474096500mole− The mass of zinc lost =molarmassofZn×moleratio×molesofelectronspassed=65.4gmol×1molZn2mole−×3474096500mole−=11.76g.