n air at 25 °C and 1.00 atm, the N2 concentration is 0.01 M and the O2 concentration is 0.033 M. The reaction N2(g) + O2(g) ⇄ 2NO(g) has Kc = 4.8 x 10-31 at 25 °C. Taking the N2 and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 38 °C, Kc = 1.0E-29. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = ____________ M
n air at 25 °C and 1.00 atm, the N2 concentration is 0.01 M and the O2 concentration is 0.033 M. The reaction N2(g) + O2(g) ⇄ 2NO(g) has Kc = 4.8 x 10-31 at 25 °C. Taking the N2 and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 38 °C, Kc = 1.0E-29. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = ____________ M
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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In air at 25 °C and 1.00 atm, the N2 concentration is 0.01 M and the O2 concentration is 0.033 M. The reaction
N2(g) + O2(g) ⇄ 2NO(g)
has Kc = 4.8 x 10-31 at 25 °C.
Taking the N2 and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 38 °C, Kc = 1.0E-29.
Make simplifying assumptions in your calculations. (Express your answer in scientific notation.)
[NO] = ____________ M
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