(d) For the reaction: H3C. H3C, CC-OH Cc=CH2 H20 H3C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (AreactG®).

(d) For the reaction: H3C. H3C, CC-OH Cc=CH2 H20 H3C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (AreactG®).

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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(16) Solid potassium chlorate decomposes into solid potassium chloride and oxygen according to the following balanced chemical equation: KCIO, (s) → KCI (s) + 3/2 O, (g) Given the enthalpy of reaction is -77.6 kl and the entropy of reaction is 494.6 3/K, the overall Gibbs free energy change for this reaction at 40.0°C is: (A) (B) (C) (D) (E) -252 k -157 kJ -1.55 x 10 kJ -232.5 kJ -97.4 kJ
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the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid according to the…
Part A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
ent/takeCovalentActivity.do?locator=assignment-take Review Topical TReforences] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x10-2 , at 1150 K: 2S03(g)2S02(g) + 02(g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K. A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K. C. s less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of O, will: A. Increase. B. Decrease. C. Remain the same, Submit Answer Retry Entire Group 8 more group attempts remaining Prev 50 hp
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 CO₂(g) -393.5 213.8 CO2(aq) -413.8 117.6 H₂O(g) -241.8 188.8 H₂O(1) -187.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, represents the st of 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 Feedback 15] ΑΣΦ Request Answer Part 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(2 314 J/K MacBook Pro P Pearson ? kJ Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions Contac
a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).
For the reaction NH,NO3(aq) –→N½0(g) + 2 H2O(1) AG° = -181.7 kJ and AH° = -149.6 kJ at 321 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 321 K. The entropy change for the reaction of 2.38 moles of NH,NO3(aq) at this temperature would be J/K.
From these two reactions at 298 K,
For the reaction NH,C(aq)NH,(2) + HCI(aq) AH =86.4 kJ and AS° = 79.1 J/K %3D The equilibrium constant for this reaction at 286.0 K is Assume that AH° and AS° are independent of temperature.
Calculate the standard entropy, ASixn, of the reaction at 25.0 °C using the table of thermodynamic properties. 3 C,H, (g) C,H,(1) ASixn J-K-l.mol-1 Calculate the standard Gibbs free energy of the reaction, AGxn. The standard enthalpy of the reaction, AHxn, is -633.1 kJ-mol-1. AGixn kJ-mol-1 Determine in which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. forward reverse neither both
Make a non-spontaneous process spontaneous A process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous. The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highly spontaneous: C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1) Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropy to argue this reaction is highly spontaneous?