MISSED THIS? Read Section19.8 (Pages 871-877); Watch IWE 19.6.Liquid methanol burns in oxygen to form gaseouscarbon dioxide and gaseous water.Substance H (kJ/mol) S° (J/(mol · K))CH, OH (1)-238.6126.8O₂(g)0205.2CO₂(g)-393.5213.8CO2(aq) -413.8117.6H₂O(g) -241.8188.8H₂O(1)-187.870.0▼Part Dwhere no represents the stoichiometric coefficients of the products, n, represents the stof the reactants, and Sº represents the standard entropies.AGxn=Calculate AG at 25°C.Express your answer in kilojoules to three significant figures.Submit=Provide Feedback15] ΑΣΦRequest AnswerPart E Complete previous part(s)[2(S° co₂(g)) + 4(S° H₂O(g))]- [2(S° CH₂OH()) + 3(S° 0₂(E[2(213.8 J/K)+4(188.8 J/K)] - [2(126.8 J/K) + 3(2314 J/KMacBook ProP Pearson?kJCopyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions Contac Gibbs free energy (G) is a measure of thespontaneity of a chemical reaction. It is thechemical potential for a reaction, and is minimizedat equilibrium. It is defined asG=H-TSwhere H is enthalpy, T is temperature, and Sisentropy.The chemical reaction that causes iron to corrodein air is given by4Fe +302 2Fe2O3in which at 298 K, AH = -1684 kJ andAS-543.7 J/K.AGrxn = 302 kJSubmitPart C✓ CorrectThis positive value for AG means that, at extremely high temperatures, the corrosion reaction will actually greverse, converting iron(III) oxide into iron and oxygen.Teq =Previous AnswersAt what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?Express your answer as an integer and include the appropriate units.► View Available Hint(s)SubmitProvide FeedbackμÃValueP PearsonUnitsReview | Constants I Periodic Ta?5 of 20Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |

Since part C and D contains different questions, we solve only part C which is first question…

MISSED THIS? Read Section 19.8 (Pages 871-877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H° (kJ/mol) S° (J/(mol-K)) CH, OH (1) -238.6 126.8 O₂(g) 0 205.2 213.8 117.6 CO₂(g) -393.5 CO,(aq) -413.8 H₂O(g) -241.8 H₂O(1) -187.8 188.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, repres of the reactants, and Sº represents the standard entropies. Calculate AG at 25°C. Express your answer in kilojoules to three significant figures. AGixn= Submit 5. ΑΣΦ 1412 314 J/K Request Answer Part E Complete previous part(s) [2(126.8 J ? kJ

MISSED THIS? Read Section 19.8 (Pages 871-877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H° (kJ/mol) S° (J/(mol-K)) CH, OH (1) -238.6 126.8 O₂(g) 0 205.2 213.8 117.6 CO₂(g) -393.5 CO,(aq) -413.8 H₂O(g) -241.8 H₂O(1) -187.8 188.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, repres of the reactants, and Sº represents the standard entropies. Calculate AG at 25°C. Express your answer in kilojoules to three significant figures. AGixn= Submit 5. ΑΣΦ 1412 314 J/K Request Answer Part E Complete previous part(s) [2(126.8 J ? kJ

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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options for all: 1. Reactants. 2. Products.
5. Calculate ΔH° for the reaction 2 C4H10 (g) + 13 O2 (g) → 10 H2O(g) + 8 CO2 (g) using the following information: (refer to image)
26. From the following information, determine AS° for the following: N(g) + O(g) NO(g) AS°=? > N2(g) + O2(g) → 2NO(g) AS°=24.8 J/K N2(g) 2N(g) AS°=115.0 J/K O2(g) 20(g) AS°=117.0 J/K
Methanogenic bacteria convert acetic acid (CH3COOH) to CO2(g) and CH4(g). ΔH°f, (kJ/mol) ΔG°f, (kJ/mol) CH3COOH -484.5 -389.9 CO2(g) -393.5 -394.4 CH4(g) -74.8 -50.8 Calculate ΔH°rxn. ΔH°rxn = ____ kJ Calculate ΔG°rxn. ΔG°rxn = ___kJ
Calculate ASº for the combustion of propane. C3H8(g) + 502(g) → 3CO2(g) + 4H20(g) Substance C3H8(g) O2{g) CO2(g) H2O(g) S° / (J/K•mol) 269.9 205.138 213.74 188.825 -72.5 J/K 100.9 J/K O72.5 J/K O -100.9 J/K O 877 J/K
JLK/m 23. Nitric oxide reacts with chlorine to form NOCI. 1. 2NO(g) + Cl2(g) → 2NOCI(g) Substance: NO(g) Cl2(g) AH° (kJ/mol) 0 90.29 at 298 K AG° (kJ/mol) 86.60 0 at 298 K S°(J/K • mol) 210.65 223.0 at 298 K What is AG°xn for this reaction at 550. K? A. -143.76 kJ/mol B. -78.78 kJ/mol C.-22.24 kJ/mol D.-10.6 kJ/mol E. 66600 kJ/mol NOCI(g) 51.71 66.07 261.60
Calculate the ∆H°ᵣ for the reaction NO(g) + O₂(g) → NO₂(g) Use the table below as a reference.
Please help. I need to undertsand how these types of problems are done
Titanium(IV) oxide is commonly used as a white paint pigment. The compound is produced by the reaction TiCl 4(g) + 2 H 2O(g)↔ TiO 2(s) + 4 HCl(g) What is ΔH° rxn (in kilojoules)? TiCl 4(g) ΔH f o = -763 kJ/molH 2O(g) ΔH f o = -241.8 kJ/mol.HCl(g) ΔH f o = -92 kJ/mol.TiO 2(s) ΔH f o = -945 kJ/mol.
Nitrogen ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) N2 (g) 0 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO (g) 90.3 86.6 210.8 NOCl (g) 51.7 66.1 261.8 NO2 (g) 33.2 51.3 240.1 N2O (g) 82.1 104.2 219.9 N2O4 (g) 9.2 97.9 304.3 N2O4 (l) -20.0 97.0 209.0 N2O5 (s) -42.0 134.0 178.0 N2H4 (l) 50.6 149.3 121.2 N2H3CH3 (l) 54.0 180.0 166.0 HNO3 (aq) -207.4 -111.3 146.4 HNO3 (l) -174.1 -80.7 155.6 HNO3 (g) -135.1 -74.7 266.4 NH4ClO4 (s) -295.0 -89.0 186.0 NH4Cl (s) -314.4 -202.9 94.6 NH4Cl (aq) -299.7 -210.5 169.9 NH4NO3 (s) -365.6 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 Oxygen ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) O2 (g) 0 0 205.1 O (g) 249.2 231.7 161.1 O3 (g)…
Find ∆H, ∆E, q, and w for the freezing of water at -10.0°C. The specific heat capacity of ice is 2.04 J/g .°C and its heat of fusion (the quantity of heat associated with melting) is -332 J/g.