For the equilibrium:

H_2 (g)+ I_2 (g)â2HI(g)

The following data apply:

âH^Â° (300K)= -9.6 kJãmolã^(-1) âS^Â° (300K)= 22.18 JK^(-1) ãmolã^(-1) âCp (500K)= -7.11 JK^(-1) ãmolã^(-1)

The latter value can be taken to be the average value between 300 K and 500 K.

Calculate the equilibrium constants KP, Kc, and Kï£ at 500 K. What would be the mole fraction of HI present at equilibrium if HI is introduced into a vessel at 10 atm pressure; how would the mole fraction change with pressure? (Hint: Only the heat capacity is at the right temperature; however, the others can be found by remembering their formulas and the fact that they are state variables)

Question

For the equilibrium: H_2 (g)+ I_2 (g)â2HI(g) The following data apply: âH^Â° (300K)= -9.6 kJãmolã^(-1) âS^Â° (300K)= 22.18 JK^(-1) ãmolã^(-1) âCp (500K)= -7.11 JK^(-1) ãmolã^(-1) The latter value can be taken to be the average value between 300 K and 500 K. Calculate the equilibrium constants KP, Kc, and Kï£ at 500 K. What would be the mole fraction of HI present at equilibrium if HI is introduced into a vessel at 10 atm pressure; how would the mole fraction change with pressure? (Hint: Only the heat capacity is at the right temperature; however, the others can be found by remembering their formulas and the fact that they are state variables)

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