1.

All the energy released from the reaction XrarrY, Delta_(r)G^(@)=-193 kJ mol^(-1) is used for oxidizing M^(+) as M^(+)rarrM^(3+)+2e^(-), E^(@)=-0.25 V Under standard conditions, the number of moles of M^(+) oxidized when one mole of X is converted to Y is [f=96500 C mol^(-1)]

Answer»


Solution :`m^(+)rarrm^(3+)+2E^(-)`
`DeltaG^(@)=-nFE^(@)" For 1 mole of "m^(+)`
`DeltaG^(@)=-2xx96500xx(-0.25)J`
`=+48250 J//"mole"=48.25KJ//"mole"`
ENERGY released by conversion of 1 mole of
`XRARRY DeltaG=-193 KJ`
Hence mole of `m^(+)` convert `(193)/(48.25)=4`


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