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Chromium metal can be plated out from an acidic solution containing CrO3 according to the following reaction:CrO3 + 6H++ 6e–  Cr + 3H2OCalculate the mass of chromium plated out by 24000 coulomb. How long will it take to plate out 1.5 gof chromium using 12.5 ampere current?

Chromium metal can be plated out from an acidic solution containing CrO3 according to the following reaction:CrO3 + 6H++ 6e–  Cr + 3H2OCalculate the mass of chromium plated out by 24000 coulomb. How long will it take to plate out 1.5 gof chromium using 12.5 ampere current?

Grade:12th pass

1 Answers

Arun
25750 Points
3 years ago
1. charge Q = 
 
where n is number of moles of the species under consideration, is the n-factor [ simply n-factor means change in oxidation number ]
 
and F is charge required to deposit 1 mole of electron i.e., 96500C
 
here, n - factor = 6
 
Charge, Q = 24000C
 
so, 24000C = n × 6 × 96500C
 
or, n = 24000/(96500 × 6) = 0.04145mol
 
now, mole = weight in gm/atomic weight
 
so, 0.04145 = weight in gm/52g/mol
 
or, weight in gm of chromium = 0.04145 × 52 = 2.1554g
 
2. number of mole of Cr = 1.5/52
 
number of mole of electron passed = 6 × 1.5/52 [ because change in oxidation of Cr is +6 ]
 
we know, 1 mole of electron is equivalent to 96500C charges.
 
so, charge required = 6 × 1.5/52 × 96500
 
= 9 × 96500/52
 
= 16702C
 
time required = charge/current
 
= 16702/12.5
 
= 1336.16 sec.
 
 

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