Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 16, Problem 23QAP
Calculate ΔG° at 82°C for reactions in which
(a)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Given the following:
P,(s) + 50,(g) → P,0,(s) A G° = – 2697.0 kJ/mol2H, (g) +0,(g) → 2H,0(g) A G° = – 457.18 kJ/mol
6H,0(g) +P_0 10(s) →4H,PO¸(1) AG° = - 428.66 kJ/mol
What is the standard free energy of formation, A Gf°, for phosphoric acid?
(A) 11243.3 kJ/mol
(B) -4497.2 kJ/mol
c) 4497.2 kJ/mol
D -11243.3 kJ/mol
Use the thermodynamic data provided below to determine the ΔGº for the reaction.
1A(s) + 4B(g) -> 1C(s) + 2D(g)
Given the following:
ΔGf° = -96.0 kJ mol-1 for substance A (s)
ΔGfº = 254.0 kJ mol-1 for substance B (g)
ΔGfº = 59.0 kJ mol-1 for substance C (s)
ΔGfº= 248.0 kJ mol-1 for substance D (g)
Provide your answer with final units of kJ and to one decimal place.
The Haber process for the production of ammonia involves the equilibriumN2(g) + 3 H2(g)⇌ 2 NH3(g)For this reaction, ΔH° = -92.38 kJ and ΔS° = -198.3 J/K. Assume that ΔH° and ΔS° for this reaction do not change withtemperature. (a) Predict the direction in which ΔG for the reaction changes with increasing temperature. (b) Calculate ΔG at25 °C and at 500 °C.
Chapter 16 Solutions
Chemistry: Principles and Reactions
Ch. 16 - Spontaneous Processes Which of the following...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - On the basis of your experience, predict which...Ch. 16 - On the basis of your experience, predict which of...Ch. 16 - In each of the following pairs, choose the...Ch. 16 - In each of the following pairs, choose the...Ch. 16 - Predict the sign of ΔS for the following: (a) a...Ch. 16 - Predict the sign of S for the following: (a)...
Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the order of the following reactions in...Ch. 16 - Predict the order of the following reactions in...Ch. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Prob. 18QAPCh. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Prob. 21QAPCh. 16 - Prob. 22QAPCh. 16 - Calculate G at 82C for reactions in which (a)...Ch. 16 - Calculate G at 72C for reactions in which (a)...Ch. 16 - Calculate G at 355 K for each of the reactions in...Ch. 16 - Calculate G at 415 K for each of the reactions in...Ch. 16 - From the values for G f given in Appendix 1,...Ch. 16 - Follow the directions of Problem 27 for each of...Ch. 16 - Use standard entropies and heats of formation to...Ch. 16 - Follow the directions of Question 29 for the...Ch. 16 - It has been proposed that wood alcohol, CH3OH, a...Ch. 16 - Prob. 32QAPCh. 16 - Sodium carbonate, also called washing soda, can be...Ch. 16 - The reaction between magnesium metal and water (l)...Ch. 16 - In the laboratory, POCl3 (phosphorus oxychloride)...Ch. 16 - Oxygen can be made in the laboratory by reacting...Ch. 16 - Phosgene, COCl2, can be formed by the reaction of...Ch. 16 - When permanganate ions in aqueous solution react...Ch. 16 - Discuss the effect of temperature change on the...Ch. 16 - Discuss the effect of temperature on the...Ch. 16 - At what temperature does G become zero for each of...Ch. 16 - Over what temperature range are the reactions in...Ch. 16 - For the reaction...Ch. 16 - For the reaction...Ch. 16 - For the decomposition of Ag2O:...Ch. 16 - Consider the following hypothetical equation...Ch. 16 - Prob. 47QAPCh. 16 - Prob. 48QAPCh. 16 - Red phosphorus is formed by heating white...Ch. 16 - Organ pipes in unheated churches develop tin...Ch. 16 - Prob. 51QAPCh. 16 - Pencil lead is almost pure graphite. Graphite is...Ch. 16 - Given the following data for sodium Na(s): S =51.2...Ch. 16 - Given the following data for bromine: Br2(l); S...Ch. 16 - Show by calculation, using Appendix 1, whether...Ch. 16 - Show by calculation whether the reaction HF(aq)...Ch. 16 - For the reaction...Ch. 16 - For the reaction...Ch. 16 - Consider the reaction 2SO2(g)+O2(g)2SO3(g) (a)...Ch. 16 - Consider the reaction AgCl(s)Ag+(aq)+Cl(aq) (a)...Ch. 16 - Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use...Ch. 16 - Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use ...Ch. 16 - Consider the following reaction at 25C:...Ch. 16 - Consider the reaction N2O(g)+NO2(g)3NO(g)K=4.41019...Ch. 16 - For the reaction...Ch. 16 - Consider the decomposition of N2O4 at 100C....Ch. 16 - Use the values for G f in Appendix 1 to calculate...Ch. 16 - Given that H f for HF(aq) is -320.1 kJ/mol and S...Ch. 16 - At 25C, a 0.327 M solution of a weak acid HX has a...Ch. 16 - A 0.250 M solution of a weak base R2NH has a pH of...Ch. 16 - Prob. 71QAPCh. 16 - Given the following standard free energies at 25°C...Ch. 16 - Natural gas, which is mostly methane, CH4, is a...Ch. 16 - Prob. 74QAPCh. 16 - When glucose, C6H12O11, is metabolized to CO2 and...Ch. 16 - Consider the following reactions at 25°C:...Ch. 16 - At 1200 K, an equilibrium mixture of CO and CO2...Ch. 16 - Prob. 78QAPCh. 16 - Prob. 79QAPCh. 16 - Prob. 80QAPCh. 16 - Prob. 81QAPCh. 16 - Carbon monoxide poisoning results when carbon...Ch. 16 - Prob. 83QAPCh. 16 - Determine whether each of the following statements...Ch. 16 - Which of the following quantities can be taken to...Ch. 16 - Fill in the blanks: (a) H° and G° become equal at...Ch. 16 - Fill in the blanks: (a) At equilibrium, G is. (b)...Ch. 16 - Prob. 88QAPCh. 16 - Consider the following reaction with its...Ch. 16 - Consider the graph below: (a) Describe the...Ch. 16 - Prob. 91QAPCh. 16 - Prob. 92QAPCh. 16 - Prob. 93QAPCh. 16 - Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7...Ch. 16 - Prob. 95QAPCh. 16 - The overall reaction that occurs when sugar is...Ch. 16 - Hydrogen has been suggested as the fuel of the...Ch. 16 - When a copper wire is exposed to air at room...Ch. 16 - Kafor acetic acid (HC2H3O2) at 25°C is 1.754105 ....Ch. 16 - Consider the reaction 2HI(g)H2(g)+I2(g)At 500C a...Ch. 16 - Prob. 101QAPCh. 16 - Consider the formation of HI(g) from H2(g) and...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 10.46 Discuss the effect of temperature change on the spontaneity of the following reactions at 1 atm. (a) Al2O3(s)+2Fe(s)2Al(s)+Fe2O3(s) H = 851.5kJ; S =38.5 J/K (b) N2H4(l)N2(g)+2H2(g) H =-50.6 kJ; S= 0.3315 kJ/K (c) SO3(g)SO2(g)+12O2(g) H = 98.9 kJ; S= 0.0939 kJ/Karrow_forwardCalculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwardWhich contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.arrow_forward
- a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forwardThe molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropyarrow_forward
- For the gaseous reaction of carbon monoxide and chlorine to form phosgene (COCl2), perform the following calculations. (a) Calculate the Δ S o at 298 K ( Δ H o = −220. kJ/mol and Δ G o = −206 kJ/mol). kJ/mol · K (b) Assuming that Δ S o and Δ H o change little with temperature, calculate Δ G o at 450. K. kJ/molarrow_forwardStearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH (C17H35COOH)2; ΔH°rxn = –172 kJ/mol The equilibrium constant for this reaction at 28°C is 2.9 × 103. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)arrow_forwardFind ΔG°rxn for the reaction: N2O(g) + NO2(g)¡ 3 NO(g) Use the following reactions with known ΔG°rxn values:2 NO(g) + O2(g)¡2 NO2(g) ΔG°rxn = -71.2 kJN2(g) + O2(g)¡2 NO(g) ΔG°rxn = +175.2 kJ2 N2O(g)¡2 N2(g) + O2(g) ΔG°rxn = -207.4 kJarrow_forward
- A reaction occurs in the left-to-right direction until it reaches equilibrium. Which of the following statements is/are completely correct for this reaction? Give some reasoning. A) At first, ΔSo of reaction > 0 but, when equilibrium is reached, ΔSo = 0. B) At first the reaction is exothermic and it continues until it is thermoneutral (ΔH = 0) C) ΔGo of reaction (which is a constant) remains negative throughout, else no reaction at all would occur. D) At first, the free energy, G > 0, but, when equilibrium is reached, G = 0. E) At first, the free energy change, ΔG < 0, but, when equilibrium is reached, ΔG = 0.arrow_forwardAt 25 °C, what is the Keq for a reaction where ΔH∘= –9.3 kJ/mol and ΔS∘= 75.5 J/mol·K?arrow_forwardCalculate ΔH for the following reaction: CH4 (g) + O2 (g) ⇌ CO2 (g) + H2O (l) Compound ΔH CH4 (g) -74.8 kJ/mol H2O (l) -285.8 kJ/mol CO2 (g) -393.5 kJ/moarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY