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Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this...

Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature Kp 150 K 1.4×10?6 175 K 4.6×10?6 200 K 3.6×10?2 225 K 1.1 250 K 15.5 Use the data to find ?H?rxn and ?S?rxn for the reaction.

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Expert Solution

Temperature                           Kp

150 K                  1.4×10?6

175 K                  4.6×10?4

200 K                  3.6×10?2

225 K                 1.1

250 K                  15.5

Arrhenius equation

ln(K2/k1) = DH0rxn/R[1/T1 - 1/T2]

k2 = 4.6*10^-4   T2= 175 k

k1 = 1.4*10^?6 , T1 = 150 k

DHrxn = x kj/mol , R = 8.314*10^-3 j.k-1.mol-1

ln((4.6*10^-4)/(1.4*10^?6)) = (x/(8.314*10^-3)((1/150)-(1/175))

ln 328.57 = x /8.314*10^-3)((6.67*10^-3)-(5.71*10^-3))

5.79 = x /8.314*10^-3)( 9.6*10^-4)

DHrxn = 50.14 kj/mol


DG0 = - RTlnKp

    = -8.314*150ln(1.4*10^?6)

    = -16.81 kj/mol

DG0 = DH0-TDS0


-16.81 = (50.14)-(298*DS)

-16.81-50.14 = -298DS

DSrxn =- 0.225 kj/mol.k

       = 225 j/mol.k

queen_honey_blossom answered 2 years ago
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