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Find the value of DeltaG^(0) and K(c) fo...

Find the value of `DeltaG^(0)` and `K_(c)` for the following reaction at 298K. `NO(g)+(1)/(2)O_(2)(g)hArrNO_(2)(g)`
Given: standard free energy of formation `(DeltaG_(f)^(0))` of `NO_(2)` and NO are 52.0 and 87.0 `kJ*mol^(-1)` respectively.

Text Solution

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`DeltaG^(0)` of a reaction`=sumDeltaG_(f)^(0)` of products `-sumDeltaG_(f)^(0)` of reactions. For the given reactions,
`DeltaG^(0)=DeltaG_(f)^(0)(NO_(2))-DeltaG_(f)^(0)(NO)-(1)/(2)DeltaG_(f)^(0)(O_(2))`
`=52.0-87.0-0.0=-35.0kJ*mol^(-1)`
We know that, `DeltaG^(0)=-RTlnK_(c)`
or, `-35xx10^(3)J*mol^(-1)=-8.314J*K^(-1)*mol^(-1)xx298KlnK_(c)`
or, `lnK_(c)=14.126" "therefore K_(c)=1.365xx10^(6)`.
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