Classify each of the reactions according to one of the four reaction types summarized in the table below.ReactionSpontaneous Process?ТурeΔΗ' (system)AS" (system) (Standard Conditions)1Exothermic, < 0Positive, > 0 Spontaneous at all temperatures. AS (universe) > 0.Exothermic, < 0Negative, < 0 Depends on relative magnitudes of AH° and AS°. Spontaneous at lower temperatures.2Endothermic, > 0Positive, > 0 Depends on relative magnitudes of AH and AS°. Spontaneous at higher temperatures.34Endothermic, > 0 Negative, < 0 Not spontaneous at any temperature. AS" (universe) <0.C,H12 O6 (s) + 6 O2(g) → 6 CO2 (g) + 6 H2O(L)a.A,H° = -673 kJ/mol-rxnA,S° = 60.4 J/K · mol-rxnO Spontaneous at all temperatures.O Spontaneous at lower temperatures.Spontaneous at higher temperatures.ONot spontaneous at any temperature.b.FeO(s) + C(graphite) → Fe(s) + CO(g)A,H° = 153.2 kJ/mol-rxnA,S' = 160.4 J/K · mol-rxnO Spontaneous at all temperatures.O Spontaneous at lower temperatures.Spontaneous at higher temperatures.ONot spontaneous at any temperature.

a) The reaction and data given is,

Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Туре AH°(system) AS" (system) (Standard Conditions) 1 Exothermic, < 0 Positive, >0 Spontaneous at all temperatures. AS°(universe) > 0. 2 Exothermic, < 0 Negative, <0 Depends on relative magnitudes of AH' and AS*. Spontaneous at lower temperatures. 3 Endothermic, > 0 Positive, > 0 Depends on relative magnitudes of AH° and AS*. Spontaneous at higher temperatures. Endothermic, > 0 Negative, <0 Not spontaneous at any temperature. AS"(universe) < 0. 4 C,H12O6 (s) + 6 O2(g) → 6 CO2(g) + 6 H,0(t) a. A‚H° = -673 kJ/mol-rxn A,s' = 60.4 J/K -· mol-rxn Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. O Not spontaneous at any temperature. b. FeO(s) + C(graphite) → Fe(s) + CO(g) A‚H' = 153.2 kJ/mol-rxn A,S' = 160.4 J/K · mol-rxn Spontaneous at all temperatures. Spontaneous at lower temperatures. Spontaneous at higher temperatures. O Not spontaneous at any temperature.

Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Туре AH°(system) AS" (system) (Standard Conditions) 1 Exothermic, < 0 Positive, >0 Spontaneous at all temperatures. AS°(universe) > 0. 2 Exothermic, < 0 Negative, <0 Depends on relative magnitudes of AH' and AS. Spontaneous at lower temperatures. 3 Endothermic, > 0 Positive, > 0 Depends on relative magnitudes of AH° and AS. Spontaneous at higher temperatures. Endothermic, > 0 Negative, <0 Not spontaneous at any temperature. AS"(universe) < 0. 4 C,H12O6 (s) + 6 O2(g) → 6 CO2(g) + 6 H,0(t) a. A‚H° = -673 kJ/mol-rxn A,s' = 60.4 J/K -· mol-rxn Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. O Not spontaneous at any temperature. b. FeO(s) + C(graphite) → Fe(s) + CO(g) A‚H' = 153.2 kJ/mol-rxn A,S' = 160.4 J/K · mol-rxn Spontaneous at all temperatures. Spontaneous at lower temperatures. Spontaneous at higher temperatures. O Not spontaneous at any temperature.

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

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 84AP

See similar textbooks

Similar questions

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
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.
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
ou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.
Reword the statement in Question 109 so that it is always true. Criticize this statement: Provided it occurs at an appreciable rate, any chemical reaction for which rG 0 will proceed until all reactants have been converted toproducts.
What is a spontaneous reaction?
What are the two ways that a final chemical state of a system can be more probable than its initial state?
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.