Calculate the standard free energy of the following reactions at 25°C, using standard free energies of formation.SubstanceAG; (kJ/mol)Al2 O3 (s)- 1582.3- 743.5Fe, O3 (8)COCL, (9)H2O(1)CO2 (g)HCl(g)- 205.9- 237.1- 394.4- 95.30a. For the reactionAl, O3 (s) + 2Fe(s) → Fe2O3 (s) + 2Al(s)Standard free energykJb. For the reactionCOCI, (g) + H2O(1) → CO2(g) + 2HC1(g)Standard free energykJSubmit AnswerTry Another Version10 item attempts remaining

Answered: Image /qna-images/answer/7c56d3cb-9825-4d1f-812a-1463677b4564.jpg

Calculate the standard free energy of the following reactions at 25°C, using standard free energies of formatio Substance AG; (kJ/mol) - 1582.3 Al, O3 (8) Fe, O3 (s) COCL, (9) H2O(1) CO2(9) - 743.5 - 205.9 - 237.1 - 394.4 HCl(9) - 95.30 a. For the reaction Al, O3 (s) + 2Fe(s) → Fe2O3 (s) + 2Al(s) Standard free energy = kJ b. For the reaction COCL2 (9) + H2O(1) → CO2 (g) + 2HCI(g) Standard free energy = kJ Submit Answer Try Another Version 10 item attempts remaining

Calculate the standard free energy of the following reactions at 25°C, using standard free energies of formatio Substance AG; (kJ/mol) - 1582.3 Al, O3 (8) Fe, O3 (s) COCL, (9) H2O(1) CO2(9) - 743.5 - 205.9 - 237.1 - 394.4 HCl(9) - 95.30 a. For the reaction Al, O3 (s) + 2Fe(s) → Fe2O3 (s) + 2Al(s) Standard free energy = kJ b. For the reaction COCL2 (9) + H2O(1) → CO2 (g) + 2HCI(g) Standard free energy = kJ Submit Answer Try Another Version 10 item attempts remaining

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

For the reaction 2HBr (9) + Cl₂ (9) - 4 2HCl(g) + Br₂ (9) =-1.2 J/K AH-81.1 kJ and AS = - The standard free energy change for the reaction of 1.52 moles of HBr (g) at 318 K, 1 atm would be [ This reaction is favored under standard conditions at 318 K. Assume that AH and AS are independent of temperature. Submit Answer Retry Entire Group 3 more group attempts remaining kj.
Consider the reaction: I2(g) + Cl2(g) 2ICI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.030 moles of I2(g) react at standard conditions. AG°rxn = kJ Submit Answer Retry Entire Group 9 more group attempts remaining
What is the standard free-energy change for the following reaction: 2C6H6 (l) + 15O2 (g) 12CO2 (g) + 6H2O (l) at 25 0C? Values of delta Gf of substances at standard conditions are as follows: Benzene = 124.5 kJ/mol, Carbon dioxide = -394.4 kJ/mol, Oxygen gas = 0.0 kJ/mol, and Liquid water =A. -237.2 kJ/mol. B. -64.05 kJC. +640.5 kJD. -6405 kJE, None of the above
Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: Al,0; (s)+3H, (g) 2Al (s)+ 3H,0 (g) Round your answer to zero decimal places. | kJ
[References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.54 x 1025 for the following reaction. CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) Topics] Based on this value of Keq: AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.73 moles of CO(g) at standard conditions at 298 K. AGO kj rxn Submit Answer Retry Entire Group 4 more group attempts remaining
Consider the reaction: C(5,graphite) + 02(g) CO2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.380 moles of C(s,graphite) react at standard conditions. AG nn kJ
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?
The decomposition of crystalline N2O5N2O5(s)?2NO2(g)+12O(g)is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ?C we have the following values for the standard state enthalpy and free energy changes of the reaction: Delta H = +109.6 kJ/mol Delta Standard Gibbs Free Energy = -30.5 kJ/mol C) Calculate delta U for this reaction at 25 C.
For the reaction CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) AH = 206.1 kJ and AS = 214.7 J/K The standard free energy change for the reaction of 1.83 moles of CH4 (9) at 345 K, 1 atm would be kj. This reaction is favored under standard conditions at 345 K. Assume that AH and AS are independent of temperature.