АPPENDI х В+Thermodynamic DataThermodynamic Data for Selected Elements and Inorganic Compoundsat 1 bar and 298 K“Substance AfĦ°/kJ · mol¯! Af&/kJ· mol¯ §/J·K-1. mol T;,/J·K-1 .mol-Ag(s)42.725.49Ag+(aq)105.977.1172.6837.66AgBr(s)-99.5-95.94107.1152.38AgCl(s)-127.0-109.7296.250.79AgI(s)-62.4-66.3114.254.43AgNO3(s)-129.4-33.41140.993.05Al(s)28.3224.34Al3+ (aq)-531.0-485-321.7AICI3(s)-704.2-628.8110.6791.84Al,O3(s)-1669.8-1576.450.9978.99Ar(g)Ba(s)Ba2+(aq)154.820.7962.826.36-537.6-560.810BaO(s)-553.5-525.170.347.45BaCl2(s)-858.6-810.9123.775.31BaSO (s)-1464.4-1353.1132.2101.75Be(s)9.5417.82BeO(s)-610.9-581.614.125.4Br2(1)152.2375.69Br (aq)-121.6-103.9682.4HBr(g)-36.4-53.45198.729.12C(graphite)5.78.52C(diamond)1.902.872.46.11CO(g)-110.5-137.3197.929.14CO2(9)-393.5-394.4213.637.1"Data are mostly from the NBS Tables of Chemical Thermodynamic Properties (1982). Thevalues for ions in aqueous solution (1 M), such as Li+(aq), are based on the convention thatall the properties listed for H+(ag) are equal to zero. Nitric oxide is an air pollutant found in car exhaust (as exhibited in the recent Volkswagenscandal). At the high temperatures found in car engines it is formed from the components of air:N2(g) + 02(g) = 2NO(g)(a) Using the data in Chang Appendix B, calculate the equilibrium constant for this reaction at25°C and 1 atm.(b) 1500°C is a typical temperature inside a car engine after it has been running for some time.Calculate the equilibrium constant for the production of nitric oxide at this higher temperature.State any assumptions you need to make in order to complete the calculation. (Even though thetemperature change is large here, assume that AHrxn, ASrxn can be treated as temperatureindependent.)

#(a): Equilibrium constant(K) and and standard Gibbs free energy are related through the following…

Nitric oxide is an air pollutant found in car exhaust (as exhibited in the recent Volkswagen scandal). At the high temperatures found in car engines it is formed from the components of air: N2(g) + 02(g) = 2NO(g) (a) Using the data in Chang Appendix B, calculate the equilibrium constant for this reaction at 25°C and 1 atm. (b) 1500°C is a typical temperature inside a car engine after it has been running for some time. Calculate the equilibrium constant for the production of nitric oxide at this higher temperature. State any assumptions you need to make in order to complete the calculation. (Even though the temperature change is large here, assume that AHrxn, ASrxn can be treated as temperature independent.)

Nitric oxide is an air pollutant found in car exhaust (as exhibited in the recent Volkswagen scandal). At the high temperatures found in car engines it is formed from the components of air: N2(g) + 02(g) = 2NO(g) (a) Using the data in Chang Appendix B, calculate the equilibrium constant for this reaction at 25°C and 1 atm. (b) 1500°C is a typical temperature inside a car engine after it has been running for some time. Calculate the equilibrium constant for the production of nitric oxide at this higher temperature. State any assumptions you need to make in order to complete the calculation. (Even though the temperature change is large here, assume that AHrxn, ASrxn can be treated as temperature independent.)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.104QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high...

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