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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.

Chemistry: The Molecular Science
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
Section16.3: Measuring Dispersal Of Energy: Entropy
Problem 16.3CE
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Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Турe ΔΗ' (system) AS" (system) (Standard Conditions) 1 Exothermic, < 0 Positive, > 0 Spontaneous at all temperatures. AS (universe) > 0. Exothermic, < 0 Negative, < 0 Depends on relative magnitudes of AH° and AS°. Spontaneous at lower temperatures. 2 Endothermic, > 0 Positive, > 0 Depends on relative magnitudes of AH and AS°. Spontaneous at higher temperatures. 3 4 Endothermic, > 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-rxn A,S° = 60.4 J/K · mol-rxn O 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-rxn A,S' = 160.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. ONot spontaneous at any temperature.
Transcribed Image Text:Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Турe ΔΗ' (system) AS" (system) (Standard Conditions) 1 Exothermic, < 0 Positive, > 0 Spontaneous at all temperatures. AS (universe) > 0. Exothermic, < 0 Negative, < 0 Depends on relative magnitudes of AH° and AS°. Spontaneous at lower temperatures. 2 Endothermic, > 0 Positive, > 0 Depends on relative magnitudes of AH and AS°. Spontaneous at higher temperatures. 3 4 Endothermic, > 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-rxn A,S° = 60.4 J/K · mol-rxn O 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-rxn A,S' = 160.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. ONot spontaneous at any temperature.
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