Chromium metal can be plated out from an acidic solution contaning CrO3 according to the following equiation- CrO3aq - 6H-aq - 6e- - Crs -3H2OThe no- of grams of chromium that will be plated out by 2400 C current is- write your answer to nearest integer

CrO_3 + 6H^⊕ + 6e^ → Cr + 3H_2O #160;(Atomic weight #160; = 52)52 g of Cr is deposited by passing electric current of 6 96500 C.(a) In the given data ...

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Standard XII

Chemistry

Nernst Equation

Chromium meta...

Question

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)

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Solution

$C r O_{3} + 6 H^{\oplus} + 6 e^{-} \to C r + 3 H_{2} O$ (Atomic weight = 52)
52 g of Cr is deposited by passing electric current of 6 96500 C.
(a) In the given data 2400 C current is passed, so amount of deposited Cr
= $\frac{52 \times 24000}{6 \times 96500} g = 2.155 g$

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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

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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

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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?

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

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Chromium metal can be plated out from an acidic solution contaning CrO3 according to the following equiation:CrO3(aq)+6H⊕(aq)+6e−→Cr(s)+3H2OThe no. of grams of chromium that will be plated out by 2400 C current is: (write your answer to nearest integer)

CrO3+6H⊕+6e−→Cr+3H2O (Atomic weight = 52)52 g of Cr is deposited by passing electric current of 6 96500 C.(a) In the given data 2400 C current is passed, so amount of deposited Cr = 52×240006×96500g=2.155g

$C r O_{3} + 6 H^{\oplus} + 6 e^{-} \to C r + 3 H_{2} O$ (Atomic weight = 52)
52 g of Cr is deposited by passing electric current of 6 96500 C.
(a) In the given data 2400 C current is passed, so amount of deposited Cr
= $\frac{52 \times 24000}{6 \times 96500} g = 2.155 g$