The following equation represents the decomposition of a generic diatomic elemen

Question

The following equation represents the decomposition of a generic diatomic element in its standard state. 1/2 X_2(g) rightarrow X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.95 kJ middot mol^-1 at 2000. K and - 50.07 kJ middot mol^-1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. At 2000. K, we were given: Delta G_f = 4.95 kJ mol^-1. What is K at that temperature? K at 2000. K = At 3000. K. we were given Delta F_f = -50.07 kJ middot mol^-1. What is K at that temperature? K at 3000. K =

Explanation / Answer

Delta G = -RT ln K

where R is universal gas constant = 8.314 J/ mol .K

and T is temperature in kelvin

So for K at 2000K

4950 = - 8.314 x 2000 ln kc

ln kc = -0.2977

kc = 0.7425

[ hint : u didnot take the inverse logarithm]

For kc at 3000 k

-50070 = -8.314 x 3000 ln kc

ln kc = 2.007

kc = 7.44

[ you have repeated the same thing here , did not take the inverse logarithm ]

hope this helps !!

let me know in the comments below ...

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