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The atmosphere contains 78% N2(g), 21% O2(g), and traces of other gases. These gases react at high temperature to form nitrogen monoxide, an important pollutant. N2(g) + O2(g) = 2NO (g) For this reaction at a certain temperature, Kc = 3.8 x 10^-5. If the initial concentration of N2(g) is 0.78 mol/L, and O2(g) is 0.21 mol/L, what will be the equilibrium concentration of NO(g) at this temperature?

The atmosphere contains 78% N2(g), 21% O2(g), and traces of other gases. These gases react at high temperature to form nitrogen monoxide, an important pollutant. N2(g) + O2(g) = 2NO (g) For this reaction at a certain temperature, Kc = 3.8 x 10^-5. If the initial concentration of N2(g) is 0.78 mol/L, and O2(g) is 0.21 mol/L, what will be the equilibrium concentration of NO(g) at this temperature?

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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
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The atmosphere contains 78% N2(g), 21% O2(g), and traces of other gases. These gases react at high temperature to form nitrogen monoxide, an important pollutant.

N2(g) + O2(g) = 2NO (g)

For this reaction at a certain temperature, Kc = 3.8 x 10^-5. If the initial concentration of N2(g) is 0.78 mol/L, and O2(g) is 0.21 mol/L, what will be the equilibrium concentration of NO(g) at this temperature?

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