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Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. 96 AF

Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. 96 AF

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.50PAE: For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then...
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der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
Transcribed Image Text:der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
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