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12 Dec 2019

The molar bond energy for O=O (double bonded oxygen molecule) is 502 kJ/mol. Calculate the standard molar entropy change for the reaction: O2 â 2 O

A) 3.37 kJ/K

B) 1.68 kJ/K

C) 502 kJ

D) 0 kJ/K

E) 32 kJ/K

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13 Dec 2019

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Given the following thermodynamic data and balanced equation, calculate the standard free energy change (delta G degree) for the reaction at 25 degree C. Also, based on the calculated (delta G degree), is the reaction spontaneous or non- spontaneous at this temperature? [delta G degree = delta H degree - (delta S degree middot T)] CH_4 (g) + 2 O_2 (g) rightarrow CI_2 (g) + 2 H_2 O(I) delta H degree = -806 kJ {delta S degree [CO_2 (g) = 213.6 J/mol middot K]}, {delta S degree [H_2 O(I) = 129.3 J/mol middot K}}, {delta S degree [CH_4 (g) = 186.2 J/mol middot K]}, {delta S degree [O_2 (g) = 205 J/mol middot K]} a) 0.0 kJ: Reaction is at Equilibrium b) 268.6 kJ: Reaction is Non-Spontaneous c) -268.6 kJ: Reaction is Spontaneous d) -806 kJ: Reaction is Spontaneous e) 806 kJ: Reaction is Non-Spontaneous Given the following thermodynamic data and balanced equation, calculate the standard free energy change (delta G degree) for the reaction at 25 degree C. Also, based on the calculated (delta G degree), is the reaction spontaneous or non-spontaneous at this temperature? [delta G degree = delta H degree - (delta S degree middot T)] 2 Mg O(s) rightarrow 2 Mg (s) + O_2 (g) delta H degree = 1203 kJ {delta S degree [Mg (s) = 32.5 J/mol middot K] }, {delta S degreeÂÂ [O_2 (g) = 205 J/mol middot K]}, {delta S degree [MgO(s) = 26.8 J/mol middot K]} a) 1139 kJ: Reaction is Non-Spontaneous b) -1139 kJ: Reaction is Spontaneous c) 216.4 kJ: Reaction is Non-Spontaneous d) -216.4 kJ: Reaction is Spontaneous e) 472 kJ: Reaction is Non-Spontaneous Ozone in the lower atmosphere is a pollutant that can form by the following reaction involving the oxidation of unburned hydrocarbons. Using the following thermodynamic data at 25 degree C, calculate the standard change in Free Energy (delta G degree) for the following reaction: CH_4(g) + 8O_2(g) rightarrow ÂCO_2(g) + 2H_2 O(g) + 4O_3(g) delta G degree = ? {delta G degree [CO_2 (g) = 394.4 kJ/mol]}, (delta G degree [H_2 O(g) = -228.6 kJ/mol]}, {delta G degree [O_3(g) = 163.2 kJ/mol]}, {delta G degree ÂÂ[CH_4 (g) =-50.5 kJ/mol]}, {delta G degree [O_2(g) = 0.0 kJ/mol]} a) -465.0 kJ b) 148.4 kJ c) -114.9 kJ d) 114.9 kJ e) -148.4 kJ

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The molar bond energy for O=O (double bonded oxygen molecule) is 502 kJ/mol. Calculate the standard molar entropy change for the reaction: O2 â 2 O

A) 3.37 kJ/K

B) 1.68 kJ/K

C) 502 kJ

D) 0 kJ/K

E) 32 kJ/K

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The molar bond energy for O=O (double bonded oxygen molecule) is 502 kJ/mol. Calculate the standard molar entropy change for the reaction: O2 â 2 O A) 3.37 kJ/K B) 1.68 kJ/K C) 502 kJ D) 0 kJ/K E) 32 kJ/K

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

The molar bond energy for O=O (double bonded oxygen molecule) is 502 kJ/mol. Calculate the standard molar entropy change for the reaction: O2 â 2 O

A) 3.37 kJ/K

B) 1.68 kJ/K

C) 502 kJ

D) 0 kJ/K

E) 32 kJ/K