The decomposition of a generic diatomic element in its standard state is represented by the equation {x,) - X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.55 kJ mol- at 2000. K and --48.71 kJ mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at cach temperature. At 2000. K, AG, = 5.55 kJ mol-, What is K at that temperature? Kat 2000. K = At 3000. K, AG = -48.71 kJ mol-I, What is K at that temperature? K at 3000. K

The decomposition of a generic diatomic element in its standard state is represented by the equation {x,) - X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.55 kJ mol- at 2000. K and --48.71 kJ mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at cach temperature. At 2000. K, AG, = 5.55 kJ mol-, What is K at that temperature? Kat 2000. K = At 3000. K, AG = -48.71 kJ mol-I, What is K at that temperature? K at 3000. K

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 108CP

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
Determine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pb
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
5.11. Determine the numerical value of Q for the reaction conditions indicated.