1.

What is the equilibrium constant, K for the following reaction at 400 K? 2NOCl (g) hArr 2NO(g)+Cl_(2)(g) DeltaH=77.2" kJ "mol^(-1) and DeltaS=122JK^(-1)mol^(-1) at 400K.

Answer»

`-3.708`
`1.95xx10^(-4)`
`2.8xx10^(4)`
`1.67xx10^(-5)`

Solution :`DeltaG=DeltaH-TDeltaS`
`=77.2-400xx122xx10^(-3)`
`=+28.4kJ" "MOL^(-1)=28400" J "mol^(-1)`
Further, `DeltaG=-2.303RTlogK`
or `28400=-2.303xx8.314xx400xxlogK`
`logK=-(28400)/(2.303xx8.314xx400)`
`logK=-3.708`
`K=`Antilog (-3.708)`=1.95xx10^(-4)`


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