Q3 (A) The reduction of iron III oxide by carbon is not spontaneous at 298K, but becomes spontaneous on heating. → 4 Fe (s) + 3 CO2 (g) (a) Use the given data in the below table to calculate the standard Gibbs energy change for the reaction at 298K. 2 Fe203 (s) + 3C (S) (b) Estimate the temperature at which the reaction just becomes equilibrium, at 1 bar pressure. CO2 (8) Fe (S) Fe2O3 C (S) -393.5 -824.2 A¡H°298 / kJ mol1 213.7 5.70 27.3 87.4 S°298 / JK' mol

Q3 (A) The reduction of iron III oxide by carbon is not spontaneous at 298K, but becomes spontaneous on heating. → 4 Fe (s) + 3 CO2 (g) (a) Use the given data in the below table to calculate the standard Gibbs energy change for the reaction at 298K. 2 Fe203 (s) + 3C (S) (b) Estimate the temperature at which the reaction just becomes equilibrium, at 1 bar pressure. CO2 (8) Fe (S) Fe2O3 C (S) -393.5 -824.2 A¡H°298 / kJ mol1 213.7 5.70 27.3 87.4 S°298 / JK' mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 88QRT: Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with...

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).
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)
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?)
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
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
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.
Carbon may exist as diamond, graphite, and other allotropes. The standard Gibbs energy of formation of diamond is 2.900 kJ mol-1, greater than that of graphite at 298 K. Predict which of these two allotropes is the more stable at this temperature.
Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation (∆Gof) of NH3 (g) is -105 kJ/mol at 304 K, calculate the equilibrium constant, K, at this temperature.To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3. K =
a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq. A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species. You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?
What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous? what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean? If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system
Calculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.
Calculate the standard Gibbs energy of the reaction at 298K, from the standard entropies and enthalpies of formation. CO(g) + CH3OH(l) yield CH3COOH(l)