I need some help understanding these thermodynamics concepts...Please be as clea

Question

I need some help understanding these thermodynamics concepts...Please be as clear as possible and show all your work. Thank You. The answers I am suppose to get are also provided (Last Image)

For the reaction below: 2 H2O (I) 2 H2 (g) + O2 (g) where Delta Gf degree for H2O (I) is -237.2 kJ/mole, calculate the standard free-energy change for this reaction and calculate K. At what temperature will the equilibrium constant for the formation of NOCI (g) be equal to 1.00 Times 10 3? Data for this reaction at 25 degree C are: 2 NO (g) + Cl2 (g) 2 NOCI (g) Delta G degree = -40.9 kJ mole1 Delta H degree = -77.1 kJ mole -1 Delta S degree = -121.3 J mole -1 k -1 (You can assume that Delta H degree and Delta S degree do not change much with temperature, but Delta G degree will.) Using the information in question #5, what is the value for the equilibrium constant at 25 degree C? At 75 degree C? At 298 K, Delta Gf degree [CO(g)] = -137.2 kJ mole1 and Kp = 6.5 Times 10 11 for the reaction CO (g) + CI2 (g) COCI2 (g). Use these data to determine Delta Gf degree[COCl2 (g)]. 6.9 Times 10-84 1.6 Times 10 -23 atm, 0.535 atm 431 K 1.5 Times 107, 1.7 Times 10 5 -205 kJ/mole

Explanation / Answer

3. Delta Go = Gf of product - Gf of reactant (Since product are element, their Gf = 0) = -2*-237.2 = 474.4 K

-RT lnK = Go = 474400 ; K = 6.954*10^-84

7. K = 6.5*10^11 ; Go = -RT ln K = -67.39 kJ

Gf [COCl2] - Gf [CO] = Go

Gf[COCl2] = -204.6 kJ

5. G = H - TS ; dG = dH - Tds - SdT ; Since, dH and dS = 0

dG = - S*dT ; (Gf - (-40900)) = 121.3 * (Tf - 298)

Also. Gf = -RTf ln K = -57.43 Tf

Solve two simultaneeous equation to get ,

Tf = 448 K

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