Question
Asked Dec 9, 2019
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A current of 3.73 A is passed through a Cr(NO,), solution. How long, in hours, would this current have to be applied to plate
out 6.90 g of chromium?
time required:
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A current of 3.73 A is passed through a Cr(NO,), solution. How long, in hours, would this current have to be applied to plate out 6.90 g of chromium? time required:

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Expert Answer

Step 1

The charge on Cr is +2. Hence 2 moles of electrons are required,

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1 mole of Cr = 52 g 52 grams = 1 mole =-x 6.90 = 0.132 moles 52 6.90 grams

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Step 2

1 mole of Cr requires 2 mole electrons; therefore 0.132 mole will require,

Moles of electron = 2 x 0.132 = 0.264 moles.

Now calculating the total charge present in 0.264 moles of electrons, this can be done as,

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1 mole consists of=96500 C 0.264 mole will consist of= 0.264 x 96500 C = 25476 C.

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Step 3

The time can be cal...

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Q=Ixt 25476 C = 3.73 C/s x t t= 6830 s = 4.74 hours

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