Part A is completed but I need help on Part B. Please and thank you II Review | Constants | Periodic TableNitric oxide, NO, also known as nitrogen monoxide, is one of theprimary contributors to air pollution, acid rain, and the depletion of theozone layer. The reaction of oxygen and nitrogen to form nitric oxide isRelation among thermodynamic quantitiesN2(9) + O2(9)→2NO(9)The heat produced by an automobile engine is sufficient to convertsome of the nitrogen and oxygen in the air to nitric oxide. Thespontaneity of a reaction can be determined from the sign of, A,GThe thermodynamic properties for a reaction are related by the equation that defines the standard Gibbs energy change of reaction, A,G", in kJ mol 1A,G° = A‚H° –TA,S°where A,H° is the standard enthalpy change in kJ mol 1 and A,S° is the standard entropy change in J K' mol 1.A good approximation to the standard Gibbsenergy change at any temperature can be obtained by using this equation assuming that A,H° and A,Sº change little with temperature.• A reaction is spontaneous when the Gibbs energychange is less than zero.• A reaction is nonspontaneous when the Gibbs energychange is greater than zero.• A reaction is in equilibrium when the Gibbs energychange is equal to zero.Part AFor the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data:A,H°182.6 kJ mol 1A;S° 24.80 J K ' mol1Calculate the temperature in kelvins above which this reaction is spontaneous.Express your answer to four significant figures and include the appropriate units.• View Available Hint(s)T = 7363 KSubmitPrevious Answersv Correct7363 K is an extremely high temperature. The combustion chamber of an automobile engine reaches only about 2400 K. Therefore, this reaction is notspontaneous even in the heat of a car's engine. How, then, can we explain why nitric oxide is produced?Relationship between Gibbs energy and the equilibrium constantThe standard Gibbs energy change, A;G", and the equilibrium constant K for a reaction can be related by the following equation:A,G = -RT In Kwhere T is the Kelvin temperature and Ris equal to 8.314 J K 1 mol 1 Nitric oxide, NO, also known as nitrogen monoxide, is one of theprimary contributors to air pollution, acid rain, and the depletion ofthe ozone layer. The reaction of oxygen and nitrogen to form nitricoxide isspontaneous even in the heat of a car's engine. How, then, can we explain why nitric oxide is produced?N. (9) + Ο (9) -2NO (9)The heat produced by an automobile engine is sufficient to convertsome of the nitrogen and oxygen in the air to nitric oxide. Thespontaneity of a reaction can be determined from the sign of, A,GRelationship between Gibbs energy and the equilibrium constantThe standard Gibbs energy change, A,G", and the equilibrium constant K for a reaction can be related by the following equation:A;G" =-RT In Kwhere T is the Kelvin temperature and Ris equal to 8.314 J K ' mol1.• A reaction is spontaneous when the Gibbs energychange is less than zero.• A reaction is nonspontaneous when the Gibbs energychange is greater than zero.• A reaction is in equilibrium when the Gibbs energychange is equal to zero.Part BCalculate the equilibrium constant for the following reaction at room temperature, 25 °C:N2(9) + O2(9)→2NO(g)Express your answer numerically to three significant figures.• View Available Hint(s)Πνα ΑΣφK = 4.411 • 10-16SubmitPrevious AnswersX Incorrect; Try Again; 5 attempts remaining

The considered reaction is, N2 (g) + O2 (g)→2NO (g)

Nitric oxide, NO, also known as nitrogen monoxide, is one of the primary contributors to air pollution, acid rain, and the depletion of the ozone layer. The reaction of oxygen and nitrogen to form nitric oxide is spontaneous even in the heat of a car's engine. How, then, can we explain why nitric oxide is produced? Relationship between Gibbs energy and the equilibrium constant N2(9) + O2(9)→2NO(g) The heat produced by an automobile engine is sufficient to convert some of the nitrogen and oxygen in the air to nitric oxide. The spontaneity of a reaction can be determined from the sign of, A,G The standard Gibbs energy change, A,G", and the equilibrium constant K for a reaction can be related by the following equation: A,G =-RT In K where Tis the Kelvin temperature and Ris equal to 8.314 J K 'mol • Areaction is spontaneous when the Gibbs energy change is less than zero. • Areaction is nonspontaneous when the Gibbs energy change is greater than zero. • Areaction is in equilibrium when the Gibbs energy change is equal to zero. Part B Calculate the equilibrium constant for the following reaction at room temperature, 25 °C: N2(9) + O2(9)→2NO(9) Express your answer numerically to three significant figures. > View Available Hint(s) να ΑΣφ K= 4.411 • 10~16 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining

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...