SATHEE: Electrochemistry - Result Question 39

Electrochemistry - Result Question 39

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

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

Calculate (i) How many grams of chromium will be plated out by $24, 000 C$ and (ii) How long will it take to plate out $1.5 g$ of chromium by using 12.5 A current?

(1993, 2M)

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Solution:

Molar mass of $C r = 52 g$

Equivalent mass of $C r = \frac{52}{6} g$

(i) Mass of Cr deposited on passing 24000 Coulombs

$= \frac{24000}{96500} \times \frac{52}{6} g = 2.15 g$

(ii) Number of gram equivalent of $C r = \frac{1.5}{52} \times 6 = \frac{9}{52}$

$\Rightarrow$ Coulombs required for $1.5 g C r = \frac{9}{52} \times 96500 = I t$

$\Rightarrow t = \frac{9 \times 96500}{52 \times 12.5} s = 22.27 m i n$

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Electrochemistry - Result Question 39

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