Use standard thermodynamic data to determine the equilibrium constant, K, for th
ID: 514657 • Letter: U
Question
Use standard thermodynamic data to determine the equilibrium constant, K, for the following reaction (note that delta G_f degree (NOCl) = +66.99 kJ/mol and others are on the hack of the periodic table): 2 NO _(g) + Cl_2 (g) 2 NOCl_(g) Calculate the Gibbs free energy change for the following reaction at 298.0 K. when the partial pressures of NO, Cl_2, and NOCl are 0.0160 bar. 0.0110 bar, and 5.26 bar, respectively. Indicate whether this reaction mixture is likely to form reactants, is likely to form products, or is at equilibrium.Explanation / Answer
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dG = dG° + RT*ln(Q)
dG° = dGproducts - dGreactants = 2*66.9 - (2*87.6 + 1*0) = -41.4 kJ = -41400
R = 8.31 J/molK
T = 298K
Q = P-NOCl^2 / (P-NO)^2(P-Cl2)
Q = (5.26^2)/((0.016^2)(0.011)) = 9825142.04545
dG = dG° + RT*ln(Q)
dG = dG° + RT*ln(Q)
dG = -41400 +8.314*298*ln(9825142.04545) = -1509.963 J/molK
dG = -1.51 kJ/mol
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