For the reaction CO(g) + Cl2(g) → COCl2(g) AG 71.4 kJ and AS137.3 J/K at 269 K and 1 atm. Reactant or Product This reaction is favored under standard conditions at 269 K. The standard enthalpy change for the reaction of 1.87 moles of CO(g) at this temperature would be kJ. For the reaction 2H2S(g) + 302(g) → 2H2O(l) +2SO2(g) AH-1124.0 kJ and AS = 390.7 J/K The standard free energy change for the reaction of 2.44 moles of H2S(g) at 295 K, 1 atm would be favored under standard conditions at 295 K. This reaction ✔ Assume that reachunt product AH° and AS are independent of temperature. kj.

For the reaction CO(g) + Cl2(g) → COCl2(g) AG 71.4 kJ and AS137.3 J/K at 269 K and 1 atm. Reactant or Product This reaction is favored under standard conditions at 269 K. The standard enthalpy change for the reaction of 1.87 moles of CO(g) at this temperature would be kJ. For the reaction 2H2S(g) + 302(g) → 2H2O(l) +2SO2(g) AH-1124.0 kJ and AS = 390.7 J/K The standard free energy change for the reaction of 2.44 moles of H2S(g) at 295 K, 1 atm would be favored under standard conditions at 295 K. This reaction ✔ Assume that reachunt product AH° and AS are independent of temperature. kj.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.104QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high...

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Similar questions

Is the following reaction spontaneous as written? Explain. Do whatever calculation is needed to answer the question. SO2(g)+H2(g)H2S(g)+O2(g)
A reaction has H298=100 kj/mol and S298=250 J/mol K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
Thermite reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat.
At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same temperature when PNO = 1.0 104 atm, PO2=2.0103 atm, and PNO2=0.30 atm. (b) Under the conditions in part a, in which direction is the reaction spontaneous?
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)
Consider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?
One of the important reactions in the biochemical pathway glycolysis is the reaction of glucose-6-phosphate (G6P) to form fructose-6-phosphate (F6P): G6PF6PG298=1.7kJ (a) Is the reaction spontaneous or nonspontaneous under standard thermodynamic conditions?. (b) Standard thermodynamic conditions imply the concentrations of G6P and F6P to be 1 M, however, in a typical cell, they are not even Close to these values. Calculate G when the concentrations of G6P and F6P are 120 M and 28 M respectively, and discuss the spontaneity of the forward reaction under these conditions. Assume the temperature is 37 C.
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25°C (b) NaCl(s)NaCl(l) at 25°C (c) 2NaCl(s)2Na(s)+Cl2(g) (d) CO2(g)C(s)+O2(g)
What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.
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?)

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