CHE330 Study Guide - Quiz Guide: Equilibrium Constant

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ceruleancoyote996

20 Mar 2015

School

University of Waterloo

Department

Chemical Engineering

Course

CHE330

Professor

Yi Feng

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10: the following reaction reaches equilibrium at 650 c and 1 bar: N2 (g) + c2h2 (g) = 2 hcn (g) The system initially is an equal molar mixture of n2 and c2h2. Determine the composition of the system at equilibrium. The standard enthalpies and gibbs energies of formation of the species and the temperature dependence of heat capacities are available in. Tables c1 and c4: consider the following two reactions that come to equilibrium at 2,000 k and 200 bar: N2 (g) + o2 (g) = no (g) N2 (g) + o2 (g) = no2 (g) (equilibrium constant k1 = 2. 004 10-2) (equilibrium constant k2 = 6. 937 10-5) Determine the mol fractions of no and no2 in the reactor when the mol fractions of n2 and. Assume ideal gases: a low-pressure, gas-phase isomerization reaction, a = b, comes to equilibrium at conditions such that vapor and liquid phases are present.

Related Questions

Consider the reaction: N₂ + 3 H₂ Â« 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 Â« 2 NH₃ .

(1 â x) 3Ã(1 â x) 2x

Let us maintain this system at a constant pressure of P_T = 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, K_p in terms of x, P_Tot and the standard pressure, P_o

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 K_p at 298.15 K. DG_f(NH₃) = -16.45 kJ/mol.

h.) From standard tables, calculate the reaction enthalpy for this reaction at 298.15 K. DH_f(NH₃) = -46.11 kJ/mol.

i.) Using your results in g.) and h.), calculate K_p 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

Calculate K at 298 K for the following reactions. Delta Gf kj/mol = NOg...... 86.60 NO2g........... 51 O2.....0 Part A : NO(g) + 1/2 O2(g)......>> NO2(g) ..(.I know the answer is 1.7 x 10^6) Part B) Use the equilibrium constant ( K= 3.89 x 10^-34 at 298K ) to calculate Delta G (in kJ) at 298 for the following reaction: 2HCL (g)....> H2 (g) + CL2 (g) answer delta G in kJ and in scientific notation please.... NOTE:... the answer to part a is correct, the answer to part b is NOT.-1.90 x 10^2 it said HInt: For any state function (G, H, or S) the change in the state function, F, for a reaction can be calculated from Delta F rxn= (sideways M)n x delta F (products) minus (sideways M) n x delta F (reactants), when n are the stoichiometric coefficients from the balanced chemical equation. Use this expression to calculate Delta G rxn. Use the expression that relates change in fuel energy of a reaction, Delta G rxn, to the equilibrium constant K. I just need part B.....thanks. View comments ...part of the answer to part B is ............10^2 Comments You commented it said ^2 not ^-2 in the answer.......sorry

CHE330 Study Guide - Quiz Guide: Equilibrium Constant

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