2) (3 pts) Classify each of the following reactions as one of the four possible type: i) spontaneous at all temperatures; ii) not spontaneous at any temperatures; iii) spontaneous at Low To, but not spontaneous at High T° and; iv) spontaneous at High T°, but not spontaneous at Low T°. A) NH4Cl (s) - t NH3 (g) + HCl (g) ; an endothermic reaction B) 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) -> ; an exothermic reaction C) 2SO2 (g) + O2 (g) → 2SO3 (g) ; an exothermic reaction Page

2) (3 pts) Classify each of the following reactions as one of the four possible type: i) spontaneous at all temperatures; ii) not spontaneous at any temperatures; iii) spontaneous at Low To, but not spontaneous at High T° and; iv) spontaneous at High T°, but not spontaneous at Low T°. A) NH4Cl (s) - t NH3 (g) + HCl (g) ; an endothermic reaction B) 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) -> ; an exothermic reaction C) 2SO2 (g) + O2 (g) → 2SO3 (g) ; an exothermic reaction Page

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 37E: Consider the decomposition of red mercury(II) oxide under standard state conditions.....

See similar textbooks

Similar questions

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.
Show by calculation, using Appendix 1, whether dissolving lead(II) chloride PbCl2(s)Pb2+(aq)+2Cl(aq) is spontaneous at 25C (a) when [ Pb2+ ]=1.0M;[ Cl ]=2.0M. (b) when [ Pb2+ ]=1.0105M;[ Cl ]=2.0105M.
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)
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
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.
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)
Explain why absolute entropies can be measured.
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.
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?)
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.
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25C (b) NaCl(s)NaCl(l) at 25C (c) 2NaCl(s)2Na(s)+Cl2(g)(d) CO2(g)C(s)+O2(g)