From the following reaction and thermodynamic data, find S° of SOCI, and the T at which the reaction becomes nonspontaneous. SO3(g) + SC₁₂(1) - SOCI₂(1) + SO2 (g) AG° =-75.2 kJ rxn kJ J Substance So mol mol-K SO, (g) -396.1 256.7 SC₁₂ (1) -50.0 184.0 SOC₁₂ (1) -245.9 so, (e) -296.9 248.2 Note: Reference the SI prefixes table for additional information.

From the following reaction and thermodynamic data, find S° of SOCI, and the T at which the reaction becomes nonspontaneous. SO3(g) + SC₁₂(1) - SOCI₂(1) + SO2 (g) AG° =-75.2 kJ rxn kJ J Substance So mol mol-K SO, (g) -396.1 256.7 SC₁₂ (1) -50.0 184.0 SOC₁₂ (1) -245.9 so, (e) -296.9 248.2 Note: Reference the SI prefixes table for additional information.

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...

See similar textbooks

Similar questions

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)
Chemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.
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?)
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.
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?
Iodine, I2, dissolves readily in carbon tetrachloride. For this process, H = 0 kJ/mol. I2(s) I2 (in CCl4 solution) What is the sign of rG? Is the dissolving process entropy-driven or enthalpy-driven? Explain briefly.
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?
Explain why absolute entropies can be measured.
Estimate the temperature range over which each of the following reactions is spontaneous. (a) 2Al(s)+3Cl2(g)2AlCl3(s) (b) 2NOCl(g)2NO(g)+Cl2(g) (c) 4NO(g)+6H2O(g)4NH3(g)+5O2(g) (d) 2PH3(g)3H2(g)+2P(g)
The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”