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Atmospheric nitrogen and oxygen react to form nitric oxide: N2(g) + O2(g) = 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and Po2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of K,?

Atmospheric nitrogen and oxygen react to form nitric oxide: N2(g) + O2(g) = 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and Po2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of K,?

Chemistry
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
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Atmospheric nitrogen and oxygen react to form nitric oxide: N2(g) + O2(g) = 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and Po2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 102 atm. What is the value of K,? %3D
Transcribed Image Text:Atmospheric nitrogen and oxygen react to form nitric oxide: N2(g) + O2(g) = 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and Po2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 102 atm. What is the value of K,? %3D
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