Consider the reaction: N2 + 3 H2 « 2 NH3 .
For this reaction 1 bar of N2 and 3 bars of H2 are introduced into a 10.0 L vessel at 455 K. From ICE diagrams, we see that at equilibrium, we have:
N2 + 3 H2 « 2 NH3 .
(1 â x) 3Ã(1 â x) 2x
Let us maintain this system at a constant pressure of PT = 4 bar.
a.) From the above ICE diagram, produce an expression in terms of the extent of reaction, x, that gives the total amount of material in the system at any point.
b.) From the above ICE diagram and your answer in a.), produce expressions for the mole fractions of each species in terms of the extent of reaction, x.
c.) From your result in b.), produce expressions for the partial pressures of each species using Daltonâs Law.
d.) From your results above, produce an expression for the equilibrium constant, Kp in terms of x, PTot and the standard pressure, Po
The Gibbs Free Energy for this system is plotted below vs âxâ the âextent of reactionâ defined above.
e.) Using the graphic above, calculate the partial pressures of all species at equilibrium.
f.) Calculate the equilibrium constant from your results at 455 K.
g.) From standard tables, calculate the standard Gibbs Free Energy for this reaction and use the result to calculate Kp at 298.15 K. DGf(NH3) = -16.45 kJ/mol.
h.) From standard tables, calculate the reaction enthalpy for this reaction at 298.15 K. DHf(NH3) = -46.11 kJ/mol.
i.) Using your results in g.) and h.), calculate Kp at 455 K and compare with your estimated result that you obtained from the graphic provided. Since the temperature is elevated and involve gases, use the extended equation that gives the proper temperature dependence on the enthalpy
Consider the reaction: N2 + 3 H2 « 2 NH3 .
For this reaction 1 bar of N2 and 3 bars of H2 are introduced into a 10.0 L vessel at 455 K. From ICE diagrams, we see that at equilibrium, we have:
N2 + 3 H2 « 2 NH3 .
(1 â x) 3Ã(1 â x) 2x
Let us maintain this system at a constant pressure of PT = 4 bar.
a.) From the above ICE diagram, produce an expression in terms of the extent of reaction, x, that gives the total amount of material in the system at any point.
b.) From the above ICE diagram and your answer in a.), produce expressions for the mole fractions of each species in terms of the extent of reaction, x.
c.) From your result in b.), produce expressions for the partial pressures of each species using Daltonâs Law.
d.) From your results above, produce an expression for the equilibrium constant, Kp in terms of x, PTot and the standard pressure, Po
The Gibbs Free Energy for this system is plotted below vs âxâ the âextent of reactionâ defined above.
e.) Using the graphic above, calculate the partial pressures of all species at equilibrium.
f.) Calculate the equilibrium constant from your results at 455 K.
g.) From standard tables, calculate the standard Gibbs Free Energy for this reaction and use the result to calculate Kp at 298.15 K. DGf(NH3) = -16.45 kJ/mol.
h.) From standard tables, calculate the reaction enthalpy for this reaction at 298.15 K. DHf(NH3) = -46.11 kJ/mol.
i.) Using your results in g.) and h.), calculate Kp at 455 K and compare with your estimated result that you obtained from the graphic provided. Since the temperature is elevated and involve gases, use the extended equation that gives the proper temperature dependence on the enthalpy
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
