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Reaction with Metals

Hydrogen pero...

Question

Hydrogen peroxide can be prepared by successive reactions :

$2 N H_{4} H S O_{4} \to H_{2} + (N H_{4})_{2} S_{2} O_{8}$ $(N H_{4})_{2} S_{2} O_{8} + 2 H_{2} O \to 2 N H_{4} H S O_{4} + H_{2} O_{2}$

The first reaction is an electrolytic reaction the second is steam distillation. What amount of current would have to be used in the first reaction to produce enough intermediate to yield 100 g pure $H_{2} O_{2}$ per hour? Assume 50% anode current efficiency.

315.36

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367.86

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412.57

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None of these

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Solution

The correct option is A $315.36$ A
moles of $H_{2} O_{2} = m o l e s o f H_{2} = \frac{100}{34}$
wt. of $H_{2} = \frac{100}{17} = Z i t$
$\frac{100}{17} = \frac{1 \times i \times 0.5 \times 3600}{96500}$
$i = 315.36 A m p .$

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