What is the standard free energy of the reaction, in kJ, at 298K for: 2D (aq) 1A (aq) + 1B (aq) <-> 1C (aq) + if AH° (A)= 76.6667 kJ/mol, AH° (B) = 90.258 kJ/mol, AH° (C) = 70.3702 kJ/mol, and AH (D) = 54.5914 kJ/mol AS° (A)= 35.9072 J/(mol K), AS° (B) = -25.5343 J/(mol K), AS (C) = -82.064 J/(mol K), and AS" (D) = 90.9047 J/(mol K)

What is the standard free energy of the reaction, in kJ, at 298K for: 2D (aq) 1A (aq) + 1B (aq) <-> 1C (aq) + if AH° (A)= 76.6667 kJ/mol, AH° (B) = 90.258 kJ/mol, AH° (C) = 70.3702 kJ/mol, and AH (D) = 54.5914 kJ/mol AS° (A)= 35.9072 J/(mol K), AS° (B) = -25.5343 J/(mol K), AS (C) = -82.064 J/(mol K), and AS" (D) = 90.9047 J/(mol K)

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...

See similar textbooks

Similar questions

Consider the reactions in the table. (a) Write the equilibrium constant in terms of activities for the chemical reaction of fire extinguishers: 2NaHCO3 (s) ↔ Na2CO3 (s) + CO2 (g) + H2O (g) ΔrH = 135.54 KJ (b) At 300 K the equilibrium constant is 3.95x10-6 for the reaction in (a), what is ΔrGo? (c) State in words: what happens to the equilibrium when temperature is increased? Then, verify by finding K for the reaction in (a) at 420 K.
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
Given the following information: F1- (aq): ΔGf° = -276.48 kJ/mol Na1+ (aq): ΔGf° = -261.87 kJ/mol 2 Na (s) + F2 (g) → 2 NaF (aq) a) Find ΔG° for this reaction using the above numbers. b) Write the expression for Qeq. (Note that NaF is a strong electrolyte!) c) Find ΔG at 325.0 K for 0.01500 atm F2 and 3.065 M NaF.
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).
A key step in the metabolism of glucose for energy is the isomerization of glucose-6-phosphate (G6P) to fructose-6-phosphate (F6P) as shown below. G6P 2 F6P At 298 K, the equilibrium constant for the isomerization is 0.510. (a) Calculate AG° at 298 K. 4.0 1.67 kJ/mol (b) Calculate AG when Q, the [F6P]/[G6P] ratio, equals 21.0. 4.0 9.21 kJ/mol (c) Calculate AG when Q = 0.800. 4.0 1.12 kJ/mol (d) Calculate Q in the cell if AG = -2.90 kJ/mol.
Determine the standard free energy change, ΔG°f , for the formation of S2−(aq) given that the ΔG°f for Ag+(aq) and Ag2S(s) are 77.1 kJ/mole and −39.5 kJ/mole respectively, and the solubility product for Ag2S(s) is 8 × 10−51.
Calculate AG° for the reaction shown below using the provided thermodynamic properties information. H2O2 (1) → 2 H2O () + O2 (g) Substance AH°; (kJ/mol) AS° (J/(mol•K)) H2O2 (1) - 187.8 232.9 H20 (1) -285.83 69.91 O2 (g) 205.0 -396.4 kJ/mol -350.5 kJ/mol -33.70 kJ/mol -1105 kJ/mol -417.2 kJ/mol
A reaction has a standard free energy change of -15.0 kJ mol-¹. What is the equilibrium constant of the reaction at 25 °C?
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 19.35 mm Hg. 2NO(g) + 02(g)→2NO2(g) AG = kJ/mol
A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ
A reaction A(aq)+B(aq)↽−−⇀C(aq)has a standard free‑energy change of −3.21 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?
A chemist fills a reaction vessel with 0.137 g calcium phosphate (Ca, (PO,) solid, 0.349 M calcium (Ca ) aqueous solution, and 0.240 M phosphate (Po,") 3- POA aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: Ca3 (PO4),(s) → 3Ca (aq) + 2PO, (aq) 4. Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ