QUESTION 15Consider the reaction:2 FeO (s) + 0.5 02 (g) → Fe203 (s)Given the following table of thermodynamic data,AHf (kJ/mol)S°(J/K-mol)FeO (s)-27360.75205.0O₂ (g)0Fe203 (s)-822.1689.96What is the value of the equilibrium constant at 298 K?Give your answer in exponential notation (NOT numerical form) using 3 significant figures.olution?

Answered: Image /qna-images/answer/9e3ca185-f332-4e5a-8463-17814646c7c1.jpg

QUESTION 15 Consider the reaction: 2 FeO (s) + 0.5 02 (g) → Fe203 (s) Given the following table of thermodynamic data, AHf (kJ/mol) Sᵒ (J/K-mol) FeO (s) -273 0 -822.16 60.75 205.0 02 (g) Fe203 (s) 89.96 What is the value of the equilibrium constant at 298 K? Give your answer in exponential notation (NOT numerical form) using 3 significant figures.

QUESTION 15 Consider the reaction: 2 FeO (s) + 0.5 02 (g) → Fe203 (s) Given the following table of thermodynamic data, AHf (kJ/mol) Sᵒ (J/K-mol) FeO (s) -273 0 -822.16 60.75 205.0 02 (g) Fe203 (s) 89.96 What is the value of the equilibrium constant at 298 K? Give your answer in exponential notation (NOT numerical form) using 3 significant figures.

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 a process with AH = -89.8 kJ and AS = -151 J/K. At what temperature will this process be at equilibrium? 450 234 760 595 378
Hello! I'm a tad confused about this question. What would be the correct answer?
Consider this reaction at equilibrium: 2 H2O2(g) = 2 H20(g) + O2(g) AH°rxn = -210 kJ/mol Which of the following disturbances will cause the reaction to shift to produce more O2(g)? (Select all that apply.) Volume of the container is reduced at constant temperature. The temperature is decreased. The temperature is increased. The partial pressure of H20(g) is decreased. Volume of the container is expanded at constant temperature. The partial pressure of H2O2(g) is increased. O O
A mixture of PbS, O2, PbO, and SO2 are mixed in a reaction vessel and allowed to reach equilibrium. 2PbS(s) + 3O2(g) ⇋ 2PbO(s) + 2SO2(g) ΔH = –839.9 kJ Predict whether the reaction will shift towards the reactants, shift toward the products, or remain unchanged upon the addition of PbS(s. a) no change b) shift toward the products c) shift towards the reactants
18
What is AS° for the following reaction? 2CI2(g) + SO2(g) → SOCI2(g) + Cl2O(g) Substance: Cl2g) SO23) SOCI23) Cl20(g) S°U/K • mol): 223.0 248.1 309.8 266.1 1270.0 J/K mol -104.8 J/K • mol 118.2J/K mol 104.8 J/K • mol -118.2 J/K • mol
What is AG for the reaction CaO (s) + CO₂(g) → CaCO3(s)? Substance CaO (s) CO₂ (g) CaCO, (s) Question 13 of 13 AG°f (kJ/mol) -603.3 -394.4 -1128.2 1 4 7 +/-
At what temperature in Kelvin does the reaction shown below reach equilibrium under standard state conditions. Report your answer to the correct sig figs. 2 NO(g) + O2(g) → 2 NO2(g) NO(g) Ozlg) NO2(g) AH°F 90.3 33.2 (kJ/mol S° 210.8 205.0 240.1 (J/K-mol) Temperature in Kelvin =
9 =+ For the reaction below AG° = + 33.0 kJ, AH° = + 92.2 kJ, and AS° =+ 198.7 J/K. Estimate the temperature at which this reaction occurs. 2 NH3(g) →N2(g) + 3H2(g) A) 0.464 K B) 166 K C) 298 K D) 464 K A B C
The ΔG°rxn for the reaction: A (g) + B (g) 2 C is +192 kJ/mol at 25 °C. What is the equilibrium constant? 9.72 x 10-6 2.61 x 10-2 2.30 x 10-34 0.986
For a particular reaction at 180.9 °C, AG = 527.78 kJ/mol, and AS = 953.96 J/(mol · K). Calculate AG for this reaction at -3.7 °C. AG = kJ/mol
) Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -73.5 149.3 -237.1