A galvanic cell is set up from a zinc bar weighing $100 g$ and $1.0 L$ of $1.0 M$ $C u S O_{4}$ solution. How long would the cell run if it is assumed to deliver a steady current of $1.0 A$ ? (Atomic mass of $Z n = 65$ )

48 h r s

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41 h r s

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21 h r s

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1 h r s

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Solution

The correct option is C $21 h r s$
$Z n + C u S O_{4} \to Z n S O_{4} + C u$

$2 m o l e s o f e l e c t r o n s a r e e x c h a n g e d .$

$m o l e s o f Z n = \frac{100}{63.5} = 1.57 m o l e s$

$m o l e s o f C u S O_{4} = 1 M \times 1 L = 1 m o l e s$

$CuSO4isinlimitingfraction.So,molesofelectronsexchangedare2moles.charge=2×96500CIf1Acurrentissuppliedtimerequired=2×96500s=2×965003600=53.6hr$

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A galvanic cell is set up from a zinc bar weighing 100 g and 1.0 L of 1.0 M CuSO4 solution. How long would the cell run if it is assumed to deliver a steady current of 1.0 A? (Atomic mass of Zn=65)

The correct option is C 21 hrsZn+CuSO4→ZnSO4+Cu 2molesofelectronsareexchanged.molesofZn=10063.5=1.57molesmolesofCuSO4=1M×1L=1moles CuSO4isinlimitingfraction.So,molesofelectronsexchangedare2moles.charge=2×96500CIf1Acurrentissuppliedtimerequired=2×96500s=2×965003600=53.6hr

A galvanic cell is set up from a zinc bar weighing $100 g$ and $1.0 L$ of $1.0 M$ $C u S O_{4}$ solution. How long would the cell run if it is assumed to deliver a steady current of $1.0 A$ ? (Atomic mass of $Z n = 65$ )