1.

The standard potential of the following cell is 0.23 V at 15^@C and 0.21V at 35^@C (Pt) H_2(g) |HCl(aq)|AgCl(s)|Ag(s) Calculate Delta H^@ and Delta S^@ for the cell reaction by assuming that these quantities remain unchanged in the range 15^@ to 35^@C

Answer»

Solution :`(DeltaG^@)_(298)=-nFE^@=-1 times 96500times 0.23=-22195 J =-22.195 kJ`
`(DELTA G^@)_(398)=-1 times 96500 times 0.21=-20265 J=-20.265 kJ`
Now we have
H^@-T DeltaS^@`
`therefore -22.195 =Delta H^@-288 Delta S^@`
and `-20.265 =Delta H^@-308.Delta S^@`
for these equations, we GET
`Delta H^@=49.98 kJ`
`Delta S^@=-96.50kJ`


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