An electric current is passed through electrolytic cells in series one containing `Ag(NO_(3))`(eq) and other `H_(2)SO_(4)` (aq). What volume of `O_(2)` measured at `25^(@)C` and `750`mm Hg pressure would be liberated form `H_(2)SO_(4)` if
(a) one mole of `Ag^(+)` is deposited from `AgNO_(3)` solution
(b) `8 xx 10^(22)` ions of `Ag^(+)` are deposited from `AgNO_(3)` solution.

Answer

(a) `V(O_(2))=6.2L` , (b). `V(O_(2))=0.823L`

Explanation

(i). Equivalents of `Ag^(+)=` Equivalent of `O_(2)`
`1=` equivalent of `O_(2)`
`therefore` mass of `O_(2)=(1)/(4)=(PV)/(RT)`
`V=(1)/(4)xx(0.081xx298xx760)/(750)=6.5lit`.
(ii). Moles of `O_(2)=("equivalent of "O_(2))/(4)=(8x10^(22)//6.023xx10^(23))/(4)=0.0332`.
`V=(0.0332xx0.0821xx298xx760)/(750)=0.823lit`