The chromium in the electrolytic solution is present as cr³⁺ will take 6.19 hours will it take to plate 18.0 kg of chromium onto the cathode if the current passed through the cell is held constant at 45.0 A.
It is given that mass is 18 kg. Converting mass into grams
18 x (1000g / 1 kg)
= 18000 g
So, 18 kg = 18000 g
Now, calculate the number of moles
No. of moles = mass of Cr / molecular mass of Cr
No. of moles = 18000 / 52 g/mole
No. of moles = 346.15 mole
For , Cr³⁺, 3 moles of electrons are required
Hence,
3 x 346.15 mole
1038.45
As 96500 C of charge are present in 1 mole of electrons. As a result, the charge held by 1038.45 mole of electrons will be determined as follows.
= 1038.45mol x 96500 C / mole
= 10.02 x 10⁷ C
As, we know that relation between charge, current and time is as follows.
Q = I x T
Current is given as 45 A
Therefore, charge is calculated
T = Q / I
T = 100.21 x 10⁶ / 45
T = 2.227 x 10⁶
As there are 3600 seconds in one 1 hour. Converting 2.227 x 10⁶ into hours are
= 2.227 x 10⁶ / 3600 sec/h
= 6.19 hours
Thus, if the current flowing through the cell is maintained constant at 45 A, we may estimate that it will take 6.19 hours to plate 18 kg of chromium onto the cathode.
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is = 47 g
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