Chromium metal can be plated out from an acidic solution containing CrO3- according to following equation- CrO3aq-6H- -6e- - Crs-3H2OHow long will it take to plate out 1-5 g of Cr by using 12-5 ampere current-

The correct option is A 1336 secWe have: w= ZQ or, w=Molar mass× I× tn× 96500 The molar mass of Cr = 62 n factor = 6 Putting the values, we ...

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Standard XII

Chemistry

Faraday's First Law

Chromium meta...

Question

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

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

How long will it take to plate out 1.5 g of Cr by using 12.5 ampere current?

1336 sec

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Solution

The correct option is A 1336 sec
We have:

$w = Z Q$

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

The molar mass of Cr $= 62$

n-factor $= 6$

Putting the values, we have:

$1.5 = \frac{62 \times 12.5 \times t}{6 \times 96500}$

so, $t = 1336 s e c$

Hence, the time required to deposit 1.5 g of Cr is $1336$ seconds.

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Similar questions

Q. 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?

Q. Chromium metal can be plated out from an acidic solution containing

C r O_{3}

according to the following reaction:

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

Calculate the mass of chromium plated out by

24000

coulomb. How long will it take to plate out

1.5 g

of chromium using

12.5

ampere current?

Q. 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^{-} \to C r (s) + 3 H_{2} O

Calculate how many grams of chromium will be placed out by

24000

coulombs (Atomic Weight of Cr

= 52

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)

Q. Chromium metal can be plated out from an
acidic solution containing

C r O_{3}

according to the following reaction:

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

Calculate the mass (m) of chromium plated out by

24000 c o u l o m b

.
Also, find the time (t) it will take to plate out

1.5 g

of chromium using

12.5 A

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Current efficiency is

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Molecular weight of

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Chromium metal can be plated out from an acidic solution containing CrO3, according to following equation. CrO3(aq)+6H++6e−→Cr(s)+3H2OHow long will it take to plate out 1.5 g of Cr by using 12.5 ampere current?

The correct option is A 1336 secWe have:w=ZQor, w=Molar mass×I×tn×96500The molar mass of Cr =62n-factor =6Putting the values, we have:1.5=62×12.5×t6×96500 so, t=1336 secHence, the time required to deposit 1.5 g of Cr is 1336 seconds.

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

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

How long will it take to plate out 1.5 g of Cr by using 12.5 ampere current?