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Faraday's First Law

Chromium meta...

Question

Chromium metal can be plated out from an acidic solution containing $C r O_{3}$ , according to the following equation.

$C r O_{3} (a q) + 6 H^{+} + 6 e^{-} \to C r (s) + 3 H_{2} O$

How many grams of chromium will be plated out by $24000$ coulombs?

0.78 g

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0.45 g

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1.2 g

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None of these

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Solution

The correct option is D None of these
We have-
$w = Z Q$

or, $w = \frac{M o l a r m a s s \times Q}{n \times 96500}$

Molar mass of $C r = 52$

n-factor $= 6$

Putting the values, we have:

$w = \frac{52 \times 24000}{6 \times 96500} = 2.56 g$

So, the mass of Cr deposited $= 2.155 g$

Hence, option D is correct.

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Similar questions

C r O_{3}

C r O_{3} (a q) + 6 H^{+} (a q) + 6 e^{-} \to C r (s) + 3 H_{2} O

24000

= 52

C r O_{3}

C r O_{3} + 6 H^{+} + 6 e^{-} \to C r + 3 H_{2} O

24000

1.5 g

12.5

C r O_{3}

C r O_{3} (a q) + 6 H^{+} + 6 e^{-} \to C r (s) + 3 H_{2} O

Chromium metal can be plated out from an acidic solution contaning $C r O_{3}$ according to the following equiation:

$C r O_{3} (a q) + 6 H^{\oplus} (a q) + 6 e^{-} \to C r (s) + 3 H_{2} O$

The no. of grams of chromium that will be plated out by 2400 C current is: (write your answer to nearest integer)

C r O_{3}

C r O_{3} + 6 H^{+} + 6 e^{-} \to C r + 3 H_{2} O

24000 c o u l o m b

1.5 g

12.5 A

40 %

C r

52 g m o l^{- 1}

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