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During electrolysis of molten CaCl2, 0.8 A current is passed through the cell for 1 hour. Calculate the mass of product formed at cathode. (Molar mass of Ca = 40 g mol inverse

During electrolysis of molten CaCl2, 0.8 A current is passed through the cell for 1 hour. Calculate the mass of product formed at cathode. (Molar mass of Ca = 40 g mol inverse

Grade:12

2 Answers

Vikas TU
14149 Points
4 years ago
Dear student 
There is similar question here ,Please refer the following link 
 
Hope this will help 
Good Luck 
Cheers 
Sharvi Shelar
13 Points
3 years ago
I= 0.8 A
T= 60 x 60= 3600 sec
Reaction at cathode is 
Ca+2 + 2e- -> Ca
Mole ratio = ½ 
Molecular mass = 40
W = I  x  T  x mole ratio x Molecular mass
      96500
W= 0.8 x 3600 x ½ x 40
         96500
W= 115200
      193000
W= 0.5698 grams
 
 

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