Calculate the entropy change in surroundings when 1.00 mol of H:0 ) is formed under standard conditions, AtH = -286 kJmol1. Industrially, methanol is synthesized using the reaction CO(g) + 2 H2(g) = CH:OH(g) Calculate the equilibrium constant at 298 K. AGP CO(g) = -137.2 kJ/mol; AGP H: (g)= 0; AGP CH:OH(g) = -162 kJ/mol

Calculate the entropy change in surroundings when 1.00 mol of H:0 ) is formed under standard conditions, AtH = -286 kJmol1. Industrially, methanol is synthesized using the reaction CO(g) + 2 H2(g) = CH:OH(g) Calculate the equilibrium constant at 298 K. AGP CO(g) = -137.2 kJ/mol; AGP H: (g)= 0; AGP CH:OH(g) = -162 kJ/mol

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

https://www.webassign.net/blb12/a-table-c.pdf ^ | Just copy and paste this in the search bar into google
Using enthalpies of formation, calculate deltaH for the following reaction at 25°C. Also calculate deltaS for this reaction from standard entropies at 25°C. Use these values to calculate deltaG for the reaction at this temperature. Species deltaHf(kJ/mol) S(J/mol⋅K) CH3OH(l) –238.7 126.8 O2(g) 0 205.0 CO2(g) –393.5 213.7 H2O(l) –285.8 69.95 2CH3OH(l) +3O2(g) --- 2CO2(g) + 4H2O(l) deltaH = kJ deltaS = J/K deltaG = kJ
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) ⇒ 2NH₂(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 PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH₂ = 0.750 atm? AG = 737 kJ/mol
Calculate the standard free-energy change AG® and the equilibrium constant K, for the following reaction at 25°C. CO(9) + 2H2 (9) CH; OH(9) AG¡ (kJ/mol) Substance CO(g) H2 (9) CHOН (9) -137.2 -162.0 AG" = kJ Ky
Calculate the standard entropy, Δ?∘rxn,ΔSrxn∘, of the reaction at 25.0 ∘C25.0 ∘C using the table of thermodynamic properties. 3C2H2(g)⟶C6H6(l) Δ?∘rxn= kJ⋅mol−1. Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −633.1 kJ⋅mol−1. Δ?∘rxn= kJ⋅mol−1 Determine in which direction the reaction is spontaneous as written at 25.0 ∘C25.0 ∘C and standard pressure. forward reverse both neither
(Q70) Using the tabulated values from the text (located in Appendix G, beginning at p. 1211) calculate (and report in kJ) the standard Gibbs free energy (AG°rxn) for the net reaction that occurs during photosynthesis: 6 H₂O (1) + 6 CO₂ (g) --> C6H12O6 (s) + 6 0₂ (g). The AG°f for glucose (C6H₁2O6) is -1273.3 kJ/mol.
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
Explain pleaseeeeeeeeeee