Question

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< Question 9 of 9 > Attempt 3 The equation represents the decomposition of a generic diatomic element in its standard state. X,(g) + X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.97 kJ.mol-1 at 2000. K and -47.91 kJ.mol-1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. K at 2000. K = K at 3000. K = Assuming that AHX is independent of temperature, determine the value of AHxn from this data. AHxn = kJ-mol-1

Answer 1

we know, AU where, RT luk Go Gibbs energy Ra Rydberg's constant I 8.314 Ilmak K = equilibrium constant 7 temperature - of 2000 K (: 4.97 63 - 4.97 X1000 I) ) 2 1 - a o & ou -RT lnk 4.97 XI ono = -8.314 x 2000 Ink 4970 .-16628 luk o – 0. 2988 = luk – 0.2985 - 2.303 log k – 0. 1297 & logk k a arking to. 1297) k . 10--1247 K -10.7A18] k ar 3000K 8 enk » » A = - Rilak – 47.91 xiooo = 1.920 = 1.920. - – 8.214 x 3000 x bak log k. 2-303 K = & antilog (0.8336) = 100.8336 x= [6.817 ] from cant groff's equation, we know :- in 6.612 ore Hoe omo) 0.7418

a les 9. 189 = 2000 3000 oHo 8.314 Allo g) 2.212 - ( 3000 - 2000 2.212 x 8.314 x 6 x 10" 1000 Ho a 110.24 x103 J/mol 110.84 kil mol Horn - 1110.34 k I molt
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