![DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state) for the reaction below is -8.6 kJ/mol. What is ao for this reaction at 37°C when [A)-0.2 M [B-0.2 M, (C]-0.4 M, and ID)-0.6 M? ABCDase A BCD 3.98 J/mol O -4.16 KJ/mol 0-13.22kJ/mol 0 6.81k/moll DI Question 4 2 pts Which one of the following statements is true? 0 if ΔG is negative, the reaction will be spontaneous. Exothermic reactions are always spontaneous. 4s is negative, the reaction wit be spontaneous If AH is positive, the reaction wil be spontaneous](http://img.homeworklib.com/questions/c216ac70-b4b2-11ea-8a45-7fc40f848bcb.png?x-oss-process=image/resize,w_560)
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![iven A+8 BDases c+0 CC] CD) A] B] mol k -8 600 Imol mol mol mo -3994 31J mol mol So, o pion](http://img.homeworklib.com/questions/c2e12d50-b4b2-11ea-93ca-5f582826f061.png?x-oss-process=image/resize,w_560)
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DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state)...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) Substance CO(NH2)2(aq) H2O(1) CO2(g) NH AH° (kJ/mol) -391.2 -285.9 -393.5 -46.19...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For a. reversible reaction at equilibrium, AG = 0. The equilibrium constant K of the reversible reaction is relate- AG"=-RTIn(K). Symbol 40" refers to thermodynamics standard condition: 298 K and 1 atm. Exercise:consider the following reaction: bo:pfoiex 2 HNO:(aq)+NO(g)- 3 NO2(g) + H2O(I) AH=+136.5 kJ; AS = +287.5 J/K a. Below what temperature does the following reaction becomes nonspontaneous? niliod sis anotsole s ob io...
Calculate the standard change in Gibbs free energy, AG , for the given reaction at 25.0...
Calculate the standard change in Gibbs free energy, AG , for the given reaction at 25.0 "C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH, CI() = NH(aq) + Cl" (aq) AGxn = kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGx. for the reaction is -9.39 kJ/mol. INH1 = Thermodynamic Properties at 298 K So 0 1 ΔΗ kJ/mol 0 105.8 -31.1 -32.6 -100.4 -127.0 -61.8 -124.4...
The standard change in Gibbs free energy is Δ?°′=7.53 kJ/mol . Calculate Δ? for this reaction...
The standard change in Gibbs free energy is Δ?°′=7.53 kJ/mol .
Calculate Δ? for this reaction at 298 K when [dihydroxyacetone
phosphate]=0.100 M and [glyceraldehyde-3-phosphate]=0.00600 M .
Thank you!
For the aqueous reaction CH2OH Н— —он SO CH-0–_0 CH -0 - 0- dihydroxyacetone phosphate = glyceraldehyde-3-phosphate the standard change in Gibbs free energy is AGⓇ' = 7.53 kJ/mol. Calculate AG for this reaction at 298 K when [dihydroxyacetone phosphate) = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00600 M AG = kJ/mol
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs...
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3H2(g) + Fe,0,($) 2Fe(s) + 3 H,0 () AGran kJ/mol Thermodynamic Properties at 298 K S° Substance Ag(s) Ag+(aq) Ag2O(s) Ag2S(s) AgBr(s) AgCl(s) AgI(S) AgNO3(s) Al(s) Al2O3(s) AlCl3(s) Ar(9) As(s) As2O5(s) AsCl3(1) Au(s) Ba(s) BaCl2(s) BaCO3(s) Bao(s) BaSO4(s) B(s) B203(s) AH kJ/mol 0 105.8 -31.1 -32.6 -100.4 -127.0 -61.8 -124.4 0 -1675.7 -704.2...
help please asap 3 Question 44 (1 point) What is the standard Gibbs free energy change...
help please asap
3 Question 44 (1 point) What is the standard Gibbs free energy change for the reaction below? 2 Au + 3 Mn2+ - 2 Au3+ + 3 Mn % reaction Ered (V) AU3+ + 30 - Au +1.50 Mn2+ + 2e -- Mn -1.18 +185 kJ 0-517 kJ 0-185 kJ -1.55 x 103 kJ +517 kJ none of these +1.55 x 103 kJ Question 43 (1 point) Which of the following statements are TRUE about an electrochemical...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) Substance CO(NH2)2(aq) H2O(1) CO2(g) NH AH° (kJ/mol) -391.2 -285.9 -393.5 -46.19...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For a. reversible reaction at equilibrium, AG = 0. The equilibrium constant K of the reversible reaction is relate- AG"=-RTIn(K). Symbol 40" refers to thermodynamics standard condition: 298 K and 1 atm. Exercise:consider the following reaction: bo:pfoiex 2 HNO:(aq)+NO(g)- 3 NO2(g) + H2O(I) AH=+136.5 kJ; AS = +287.5 J/K a. Below what temperature does the following reaction becomes nonspontaneous? niliod sis anotsole s ob io...
Calculate the standard change in Gibbs free energy, AG , for the given reaction at 25.0 "C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH, CI() = NH(aq) + Cl" (aq) AGxn = kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGx. for the reaction is -9.39 kJ/mol. INH1 = Thermodynamic Properties at 298 K So 0 1 ΔΗ kJ/mol 0 105.8 -31.1 -32.6 -100.4 -127.0 -61.8 -124.4...
The standard change in Gibbs free energy is Δ?°′=7.53 kJ/mol .
Calculate Δ? for this reaction at 298 K when [dihydroxyacetone
phosphate]=0.100 M and [glyceraldehyde-3-phosphate]=0.00600 M .
Thank you!
For the aqueous reaction CH2OH Н— —он SO CH-0–_0 CH -0 - 0- dihydroxyacetone phosphate = glyceraldehyde-3-phosphate the standard change in Gibbs free energy is AGⓇ' = 7.53 kJ/mol. Calculate AG for this reaction at 298 K when [dihydroxyacetone phosphate) = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00600 M AG = kJ/mol
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3H2(g) + Fe,0,($) 2Fe(s) + 3 H,0 () AGran kJ/mol Thermodynamic Properties at 298 K S° Substance Ag(s) Ag+(aq) Ag2O(s) Ag2S(s) AgBr(s) AgCl(s) AgI(S) AgNO3(s) Al(s) Al2O3(s) AlCl3(s) Ar(9) As(s) As2O5(s) AsCl3(1) Au(s) Ba(s) BaCl2(s) BaCO3(s) Bao(s) BaSO4(s) B(s) B203(s) AH kJ/mol 0 105.8 -31.1 -32.6 -100.4 -127.0 -61.8 -124.4 0 -1675.7 -704.2...
help please asap
3 Question 44 (1 point) What is the standard Gibbs free energy change for the reaction below? 2 Au + 3 Mn2+ - 2 Au3+ + 3 Mn % reaction Ered (V) AU3+ + 30 - Au +1.50 Mn2+ + 2e -- Mn -1.18 +185 kJ 0-517 kJ 0-185 kJ -1.55 x 103 kJ +517 kJ none of these +1.55 x 103 kJ Question 43 (1 point) Which of the following statements are TRUE about an electrochemical...
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