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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

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

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.101PAE
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Part A is completed but I need help on Part B. Please and thank you 

II Review | Constants | Periodic Table 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 Relation among thermodynamic quantities N2(9) + O2(9)→2NO(9) 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 thermodynamic properties for a reaction are related by the equation that defines the standard Gibbs energy change of reaction, A,G", in kJ mol 1 A,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 Gibbs energy 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 energy change is less than zero. • A reaction is nonspontaneous when the Gibbs energy change is greater than zero. • A reaction is in equilibrium when the Gibbs energy change is equal to zero. Part A For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: A,H° 182.6 kJ mol 1 A;S° 24.80 J K ' mol1 Calculate 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 K Submit Previous Answers v Correct 7363 K is an extremely high temperature. The combustion chamber of an automobile engine reaches only about 2400 K. Therefore, this reaction is not 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 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 T is the Kelvin temperature and Ris equal to 8.314 J K 1 mol 1
Transcribed Image Text:II Review | Constants | Periodic Table 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 Relation among thermodynamic quantities N2(9) + O2(9)→2NO(9) 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 thermodynamic properties for a reaction are related by the equation that defines the standard Gibbs energy change of reaction, A,G", in kJ mol 1 A,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 Gibbs energy 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 energy change is less than zero. • A reaction is nonspontaneous when the Gibbs energy change is greater than zero. • A reaction is in equilibrium when the Gibbs energy change is equal to zero. Part A For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: A,H° 182.6 kJ mol 1 A;S° 24.80 J K ' mol1 Calculate 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 K Submit Previous Answers v Correct 7363 K is an extremely high temperature. The combustion chamber of an automobile engine reaches only about 2400 K. Therefore, this reaction is not 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 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 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 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? N. (9) + Ο (9) -2NO (9) 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 Relationship between Gibbs energy and the equilibrium constant 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 T is the Kelvin temperature and Ris equal to 8.314 J K ' mol1. • A reaction is spontaneous when the Gibbs energy change is less than zero. • A reaction is nonspontaneous when the Gibbs energy change is greater than zero. • A reaction 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(g) Express your answer numerically to three significant figures. • View Available Hint(s) Πνα ΑΣφ K = 4.411 • 10-16 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining
Transcribed Image Text: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? N. (9) + Ο (9) -2NO (9) 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 Relationship between Gibbs energy and the equilibrium constant 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 T is the Kelvin temperature and Ris equal to 8.314 J K ' mol1. • A reaction is spontaneous when the Gibbs energy change is less than zero. • A reaction is nonspontaneous when the Gibbs energy change is greater than zero. • A reaction 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(g) Express your answer numerically to three significant figures. • View Available Hint(s) Πνα ΑΣφ K = 4.411 • 10-16 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining
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