A Galvanic cell is set up from a Zinc bar weighing 100g and 1L of 1M $C u S O_{4}$ solution. How long would the cell run assuming it delivers a steady current of 1 amp?

24.6 hr

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26.8 hr

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53.6 hr

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16.8 hr

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Solution

The correct option is C 53.6 hr
Moles of $Z n = \frac{100}{36.4} = 1.53$
Moles of Cu is in $C u S O_{4}$ = 1 mole
1 mole of $C u S O_{4}$ can produce = 2 $\times$ 96500C
$∴ T i m e = \frac{2 \times 96500}{1 \times 2} = 53.6 h r$

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A Galvanic cell is set up from a Zinc bar weighing 100g and 1L of 1M CuSO4 solution. How long would the cell run assuming it delivers a steady current of 1 amp?

The correct option is C 53.6 hrMoles of Zn=10036.4=1.53 Moles of Cu is in CuSO4 = 1 mole 1 mole of CuSO4can produce = 2 × 96500C ∴Time=2×965001×2=53.6 hr

A Galvanic cell is set up from a Zinc bar weighing 100g and 1L of 1M $C u S O_{4}$ solution. How long would the cell run assuming it delivers a steady current of 1 amp?

The correct option is C 53.6 hr
Moles of $Z n = \frac{100}{36.4} = 1.53$
Moles of Cu is in $C u S O_{4}$ = 1 mole
1 mole of $C u S O_{4}$ can produce = 2 $\times$ 96500C
$∴ T i m e = \frac{2 \times 96500}{1 \times 2} = 53.6 h r$