An acidic solution of `Cu^(2+)` salt contaning `0.4` of `Cu^(2+)` is electrolyzed untill all the copper is deposited. The electrolysis is continued for seven more minutes with the volume of solution kept at 100mL and the current at `1.2` amp. Calculate the volume of gases evolved at NTP during the entire electrolysis.

Options

A. 78.20 ml, 99.78 ml
B. 58.48 ml, 78.20 ml
C. 99.23ml, 58.46 ml
D. 78.20 ml, 58.48 ml

Answer

C

Explanation

No. of equivalent of `Cu^(+2)`
deposited `=(0.4 xx 2)/(63.5) = 0.013`
`:.` volume of `O_(2)` liberated at anode `=0.013 xx 5.6 = 0.07` lt `=70ml`
After continuation of electrolysis for seven more minutes
`Q = it = 1.2 xx 7 xx 60 = 504C`
Therefore, Volume of `H_(2)` liberated at cathode
`= 0.00522 xx 11200 = 58.46` ml
vol of `O_(2)` liberated at anode
`=0.00522 xx 5600 = 29.23 ml`
Total volume of gases liberated during the entire electrolysis
Oxygen `=70 +29.23 = 99.23 ml`
Hydrogen `=58.46ml`