Classify each of the reactions according to one of the four reaction types summarized in the table below.ReactionSpontaneous Process?ТуреΔΗ' (system)AS (system) (Standard Conditions)1Exothermic, < 0Positive, > 0 Spontaneous at all temperatures. AS (universe) > 0.Exothermic, < 0Negative, <0 Depends on relative magnitudes ofAH° and AS°. Spontaneous at lower temperatures.Endothermic, > 0Positive, > 0 Depends on relative magnitudes of AH and AS". Spontaneous at higher temperatures.3Endothermic, > 0 Negative, < o Not spontaneous at any temperature. AS° (universe) < 0.4C6 H12O6 (s) + 6 02 (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.O Spontaneous at higher temperatures.ONot spontaneous at any temperature.b.ВаО(s) + C(graphite) — Ba(s) + СО(g)A,H° = 437.6 kJ/mol-rxnA,S° = 184.9 J/K· mol-rxnOSpontaneous at all temperatures.O Spontaneous at lower temperatures.O Spontaneous at higher temperatures.ONot spontaneous at any temperature.

Spontaneous reaction :- A reaction which takes place on its own without the need of any external…

Reaction Spontaneous Process? Туре 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 ofAH° and AS°. Spontaneous at lower temperatures. 2 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. Cg H12O6 (s) + 6 02(g) → 6 CO2(g) + 6 H2O(£) a. A,H° = -673 kJ/mol-rxn A,S° = 60.4 J/K· mol-rxn OSpontaneous at all temperatures. OSpontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature. b. BaO(s) + C(graphite) → Ba(s) + CO(g) A,H° = 437.6 kJ/mol-rxn A,S° = 184.9 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. OSpontaneous at higher temperatures. ONot spontaneous at any temperature.

Reaction Spontaneous Process? Туре 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 ofAH° and AS°. Spontaneous at lower temperatures. 2 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. Cg H12O6 (s) + 6 02(g) → 6 CO2(g) + 6 H2O(£) a. A,H° = -673 kJ/mol-rxn A,S° = 60.4 J/K· mol-rxn OSpontaneous at all temperatures. OSpontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature. b. BaO(s) + C(graphite) → Ba(s) + CO(g) A,H° = 437.6 kJ/mol-rxn A,S° = 184.9 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. OSpontaneous at higher temperatures. ONot spontaneous at any temperature.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The energy produced by a spontaneous reaction is often used to provide the energy to drive nonspontaneous reactions. For example, the conversion of ATP to ADP in our cells acts as the energy source for the nonspontaneous reactions that combine amino acids during protein synthesis. Here is the conversion of ATP to ADP: ATP(aq) + H,O = ADP(aq) + HPO,²-(aq) AG° = -30.0 kj/mol A typical reaction combining two amino acids during protein synthesis has a AG = 15.0 kJ/mol. What is the minimum ATP concentration required to provide the energy to combine 1 mole of amino acid synthesis (total energy = 15.0 kJ)? Assume that the concentration of ADP = 9 µM (micromolar) and HPO42- = 4 mM (millimolar). %3! %3D
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A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 105.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
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