1.

The value of log_(10) K for a reaction A iff B is (Given :Delta_(r)H_(298K)^(@)=-54.07 kJ mol^(-1),Delta_(r)S_(298 K)^(@)=10 JK^(-1) mol^(-1) and R=8.314 JK^(-) mol^(-1), 2.303 xx 8.314xx298=5705)

Answer»

5
10
95
100

Solution :`A IFF B`
`DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`DeltaG^(@)=0-2.303 RT log_(10)K`
`-2.303 RT log_(10)K=DeltaH^(@)-TDeltaS^(@)`,
`2.303 RT log_(10) K=TDeltaS^(@)-DeltaH^(@)`
`log_(10)K=(TDeltaS^(@)-DeltaH^(@))/(2.303 RT)=(298xx10+54.07xx1000)/(2.303xx8.314xx298)=10`.


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