General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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
bartleby

Videos

Question
Book Icon
Chapter 18, Problem 18.85QP
Interpretation Introduction

Interpretation:

For the given reaction the values of ΔHo,ΔSoandΔGo has to be calculated and also the spontaneity of the reaction has to be explained.

Concept introduction:

Standard free energy change:

Standard free energy change is measured by subtracting the product of temperature and standard entropy change from the standard enthalpy change of a system.

ΔGo=ΔHo-TΔSowhere,ΔGo-standardfreeenergy changeΔHo-standardenthalpychangeΔSo-standardentropy changeand T-temperature.

Spontaneous process:

The chemical or physical change can takes place by itself without the help of surroundings are called as spontaneous process.

To calculate: the values of ΔHo,ΔSoandΔGo

Blurred answer
Students have asked these similar questions
Using reaction free energy to predict equilibrium composition Consider the following equilibrium: N2O4 (g) 2NO2 (g) AG⁰ = 5.4 kJ Now suppose a reaction vessel is filled with 1.68 atm of dinitrogen tetroxide (N204) at 148. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N2O4 tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO 2 needed to reverse it. Round your answer to 2 significant digits. yes no 0.42 atm ☑ 5 0/5 ? مله Ar
Homework 13 (Ch17) Question 4 of 4 (1 point) | Question Attempt: 2 of 2 ✓ 1 ✓ 2 = 3 4 Time Remaining: 4:25:54 Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: 2CH3OH (g)+302 (g) → 2CO2 (g) + 4H₂O (g) Round your answer to zero decimal places. ☐ kJ x10 ☐ Subm Check 2020 Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce
Identifying the major species in weak acid or weak base equilibria Your answer is incorrect. • Row 2: Your answer is incorrect. • Row 3: Your answer is incorrect. • Row 6: Your answer is incorrect. 0/5 The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. acids: HF 0.1 mol of NaOH is added to 1.0 L of a 0.7M HF solution. bases: 0.13 mol of HCl is added to 1.0 L of a solution that is 1.0M in both HF and KF. Exponent other: F acids: HF bases: F other: K 1 0,0,... ? 000 18 Ar

Chapter 18 Solutions

General Chemistry - Standalone book (MindTap Course List)

Ch. 18.6 - Prob. 18.9ECh. 18.6 - Prob. 18.3CCCh. 18.7 - Consider the decomposition of dinitrogen...Ch. 18.7 - The thermodynamic equilibrium constant for the...Ch. 18.7 - To what temperature must magnesium carbonate be...Ch. 18 - What is a spontaneous process? Give three examples...Ch. 18 - Which contains greater entropy, a quantity of...Ch. 18 - State the second law of thermodynamics.Ch. 18 - The entropy change S for a phase transition equals...Ch. 18 - Describe how the standard entropy of hydrogen gas...Ch. 18 - Describe what you would look for in a reaction...Ch. 18 - Define the free energy G. How is G related to H...Ch. 18 - What is meant by the standard free-energy change G...Ch. 18 - Prob. 18.9QPCh. 18 - Prob. 18.10QPCh. 18 - Prob. 18.11QPCh. 18 - Prob. 18.12QPCh. 18 - Prob. 18.13QPCh. 18 - Prob. 18.14QPCh. 18 - Prob. 18.15QPCh. 18 - Prob. 18.16QPCh. 18 - Prob. 18.17QPCh. 18 - You run a reaction that has a negative entropy...Ch. 18 - Prob. 18.19QPCh. 18 - Given the following information at 25C, calculate...Ch. 18 - Prob. 18.21QPCh. 18 - Prob. 18.22QPCh. 18 - For each of the following statements, indicate...Ch. 18 - Which of the following are spontaneous processes?...Ch. 18 - Prob. 18.25QPCh. 18 - Predict the sign of the entropy change for each of...Ch. 18 - Hypothetical elements A(g) and B(g) are introduced...Ch. 18 - Prob. 18.28QPCh. 18 - Prob. 18.29QPCh. 18 - Describe how you would expect the spontaneity (G)...Ch. 18 - Chloroform, CHCl3, is a solvent and has been used...Ch. 18 - Diethyl ether (known simply as ether), (C2H5)2O,...Ch. 18 - The enthalpy change when liquid methanol. CH3OH,...Ch. 18 - The heat of vaporization of carbon disulfide, CS2,...Ch. 18 - Predict the sign of S, if possible, for each of...Ch. 18 - Predict the sign of S, if possible, for each of...Ch. 18 - Calculate S for the following reactions, using...Ch. 18 - Calculate S for the following reactions, using...Ch. 18 - Calculate S for the reaction...Ch. 18 - What is the change in entropy, S, for the reaction...Ch. 18 - Using enthalpies of formation (Appendix C),...Ch. 18 - Using enthalpies of formation (Appendix C),...Ch. 18 - The free energy of formation of one mole of...Ch. 18 - The free energy of formation of one mole of...Ch. 18 - Calculate the standard free energy of the...Ch. 18 - Calculate the standard free energy of the...Ch. 18 - On the basis of G for each of the following...Ch. 18 - For each of the following reactions, state whether...Ch. 18 - Calculate H and G for the following reactions at...Ch. 18 - Calculate H and G for the following reactions at...Ch. 18 - Consider the reaction of 2 mol H2(g) at 25C and 1...Ch. 18 - Consider the reaction of 1 mol H2(g) at 25C and 1...Ch. 18 - What is the maximum work that could be obtained...Ch. 18 - What is the maximum work that could be obtained...Ch. 18 - Give the expression for the thermodynamic...Ch. 18 - Write the expression for the thermodynamic...Ch. 18 - What is the standard free-energy change G at 25C...Ch. 18 - What is the standard free-energy change G at 25C...Ch. 18 - Calculate the standard free-energy change and the...Ch. 18 - Calculate the standard free-energy change and the...Ch. 18 - Obtain the equilibrium constant Kc at 25C from the...Ch. 18 - Calculate the equilibrium constant Kc at 25C from...Ch. 18 - Use data given in Tables 6.2 and 18.1 to obtain...Ch. 18 - Use data given in Tables 6.2 and 18.1 to obtain...Ch. 18 - Sodium carbonate, Na2CO3, can be prepared by...Ch. 18 - Oxygen was first prepared by heating mercury(II)...Ch. 18 - Prob. 18.67QPCh. 18 - The combustion of acetylene, C2H2, is a...Ch. 18 - Prob. 18.69QPCh. 18 - Prob. 18.70QPCh. 18 - Acetic acid, CH3COOH, freezes at 16.6C. The heat...Ch. 18 - Acetone, CH3COCH3, boils at 56C. The heat of...Ch. 18 - Prob. 18.73QPCh. 18 - Prob. 18.74QPCh. 18 - Prob. 18.75QPCh. 18 - Ethanol burns in air or oxygen according to the...Ch. 18 - Acetic acid in vinegar results from the bacterial...Ch. 18 - Prob. 18.78QPCh. 18 - Is the following reaction spontaneous as written?...Ch. 18 - Is the following reaction spontaneous as written?...Ch. 18 - Prob. 18.81QPCh. 18 - The reaction N2(g)+3H2(g)2NH3(g) is spontaneous at...Ch. 18 - Prob. 18.83QPCh. 18 - Calculate G at 25C for the reaction...Ch. 18 - Prob. 18.85QPCh. 18 - Consider the reaction CS2(g)+4H2(g)CH4(g)+2H2S(g)...Ch. 18 - Prob. 18.87QPCh. 18 - a From a consideration of the following reactions,...Ch. 18 - For the reaction CH3OH(l)+32O2(g)2H2O(l)+CO2(g)...Ch. 18 - Prob. 18.90QPCh. 18 - Prob. 18.91QPCh. 18 - Tungsten is usually produced by the reduction of...Ch. 18 - For the decomposition of formic acid,...Ch. 18 - Prob. 18.94QPCh. 18 - For the reaction 2Cu(s)+S(s)Cu2S(s) H and G are...Ch. 18 - Prob. 18.96QPCh. 18 - When 1.000 g of gaseous butane, C4H10, is burned...Ch. 18 - When 1.000 g of ethylene glycol, C2H6O2, is burned...Ch. 18 - a Calculate K1, at 25C for phosphoric acid:...Ch. 18 - a Calculate K1, at 25C for sulfurous acid:...Ch. 18 - The direct reaction of iron(III) oxide. Fe2O3, to...Ch. 18 - Prob. 18.102QPCh. 18 - Prob. 18.103QPCh. 18 - Prob. 18.104QPCh. 18 - Prob. 18.105QPCh. 18 - Cobalt(II) chloride hexahydrate, CoCl26H2O, is a...Ch. 18 - Prob. 18.107QPCh. 18 - Hydrogen gas and iodine vapor react to produce...Ch. 18 - Silver carbonate, Ag2CO3, is a light yellow...Ch. 18 - Prob. 18.110QPCh. 18 - Adenosine triphosphate, ATP, is used as a...Ch. 18 - Prob. 18.112QPCh. 18 - Prob. 18.113QPCh. 18 - Prob. 18.114QPCh. 18 - Sodium acetate crystallizes from a supersaturated...Ch. 18 - According to a source, lithium peroxide (Li2O2)...Ch. 18 - Tetrachloromethane (carbon tetrachloride), CCl4,...Ch. 18 - Prob. 18.118QPCh. 18 - Prob. 18.119QPCh. 18 - Prob. 18.120QPCh. 18 - Prob. 18.121QPCh. 18 - Coal is used as a fuel in some electric-generating...Ch. 18 - Hydrogen bromide dissociates into its gaseous...Ch. 18 - Hydrogen gas and iodine gas react to form hydrogen...Ch. 18 - Prob. 18.125QPCh. 18 - Prob. 18.126QPCh. 18 - Ka for acetic acid at 25.0C is 1754 105. At...Ch. 18 - Ksp for silver chloride at 25.0C is 1.782 1010....
Knowledge Booster
Background pattern image
Chemistry
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
SEE MORE QUESTIONS
Recommended textbooks for you
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
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
Text book image
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Text book image
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Text book image
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Text book image
Introductory Chemistry For Today
Chemistry
ISBN:9781285644561
Author:Seager
Publisher:Cengage
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