Answered: The chemical reaction that causes iron…

The chemical reaction that causes iron to corrode in air is given by 4Fe+302 2Fe203 with AHrxn = -1684 kJ/mol AGrxn-1522 kJ/mol a) What is the Gibbs free energy of this process at 2500 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

Can you help me figure this out?
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
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 = .002 Carbonic acid then ionizes in water (Kal = 4.5 x 10-7). Ignoring Ka2, estimate K for the overall process by which CO, and H,0 form H* and HCO, . К — Incorrect What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Pco, atm Incorrect
Consider the following reaction; A(g) + B(g) → c(s) + D(g); AH = 159.1 kJ; AG = 164.1kJ at 298 K %3D The reaction is spontaneous at relatively high temperatures only The reaction is spontaneous at all temperatures The reaction is nonspontaneous at all temperatures. The reaction is at equilibrium at 298 K The reaction is spontaneous at relatively low temperatures only
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?
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
Calculate the free energy change under nonstandard state conditions. Use standard thermodynamic data (in the Chemistry References) to calculate triangleG at 298.15 K for the following reaction, assuming that all gases have a pressure of 10.35 mm Hg. 2S02(g) + O2(g) 2SO3(g) triangleG= kJ/mol Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. C2H4(g) + H2O(g)——->CH3CH2OH(g)
Calculate the standard free energy for the reaction given. 2 CH 3OH( l) + 3 O 2( g) → 2 CO 2( g) + 4 H 2O( l) a -797.8 kJ b -2069.8 kJ c -1404.8 kJ d -465.2 kJ
Explain pleaseeeeeeeeeee
ST5A.2 - Calculate the equilibrium constant given that the standard Gibbs free energy of reaction is -8.16 kJ/mol at 249 K for the reaction. Type your answer...