The chemical reaction that causes chromium to corrode in air is given by 4Cr(s) + 30z(9)→2C1;O3(s) What is the standard Gibbs energy change for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. and • View Available Hint(s) - 2256 kJ mol 4,s° = - 549.1 JK-' mol-' Templetes Symbols undo redo fesel kayboard shortouts Heip expofent subscript fraction dot soentfic nolabon dejete Close keyboa k•J |mol A,G^ (298 K) = 214.95 This unit is not recognized. See the list of accectable units. No credit lost. Try again. Submit Previous Anewere Part B What is the Gibbs energy for this reaction at 4717 K ? Assume that A,H° and A,S® do not change with temperature. Express your answer to two decimal places and include the appropriate units. • View Available Hint(s) Tempietes Symbols undo redo feset keyboard shortcuts Help 4,G° (4717K) = Value Units Submit

The chemical reaction that causes chromium to corrode in air is given by 4Cr(s) + 30z(9)→2C1;O3(s) What is the standard Gibbs energy change for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. and • View Available Hint(s) - 2256 kJ mol 4,s° = - 549.1 JK-' mol-' Templetes Symbols undo redo fesel kayboard shortouts Heip expofent subscript fraction dot soentfic nolabon dejete Close keyboa k•J |mol A,G^ (298 K) = 214.95 This unit is not recognized. See the list of accectable units. No credit lost. Try again. Submit Previous Anewere Part B What is the Gibbs energy for this reaction at 4717 K ? Assume that A,H° and A,S® do not change with temperature. Express your answer to two decimal places and include the appropriate units. • View Available Hint(s) Tempietes Symbols undo redo feset keyboard shortcuts Help 4,G° (4717K) = Value Units Submit

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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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
Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +20₂(g) → M₂O4(s) For this reaction, AH = -4.961 kJ/mol and AS ixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGixn= What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O₂(g) over M(s) at 298 K? MacBook Pro tyne URI + kJ/mol O
Use the data provided in the table to calculate the change in Gibbs Free-Energy at 25 degrees Celsius for the reaction given. Ag+ (aq) Cl- (aq) AgCl (s) S0 (J K-1 mole-1) 72.68 56.4 96.2 Delta H Kj/mol 105.58 -167.2 -127.07 Group of answer choices -75.2 kJ +55.7 kJ +32.5 kJ -75.2 kJ -55.7 kJ
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) 2 NH,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, Pi, = 0.100 atm, and PNH, = 0.600 atm? AG = kJ/mol
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) = 2 NH,(g) the standard change in Gibbs free energy is AG° = –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, PH, = 0.500 atm, and PNH, = 0.600 atm? AG = kJ/mol
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Carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H,O(1) -237.1 CO,(g) -394.4 K = Carbonic acid then ionizes in water (K = 4.5 x 10-7). Ignoring K2, estimate K for the overall process by which CO, and H,O form H* and HCO,. K = What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Роо, atm
For a certain chemical reaction, the standard Gibbs free energy of reaction is -133. kJ. Calculate the temperature at which the equilibrium constant K = 8.2 x 10- 22 Round your answer to the nearest degree. T= \| °C
For the following reaction : H2 (g) + I2 (g) 2HI (g) it was found that a 13.0L vessel at equilibrium contained 0.852 mol H2, 0.361 mol I2, and 2.99 mol of HI. A) Write an expression for Kc. B). Determine the value of Kc for this reaction.
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What is the value of the equilibrium constant when ΔGorxn = 25 kJ·mol-1 and T=298 K?