At 2200ºC, Kp = 0.050 for the reaction N2(g) + O2(g) -> 2NO(g) What is the partial pressure (atm) of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of 0.40 and 1.60 atm, respectively?
At 2200ºC, Kp = 0.050 for the reaction N2(g) + O2(g) -> 2NO(g) What is the partial pressure (atm) of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of 0.40 and 1.60 atm, respectively?
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter16: Thermodynamics
Section: Chapter Questions
Problem 50E: Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial...
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Transcribed Image Text:At 2200ºC, Kp
=
0.050 for the reaction N2(g) + O2(g) -> 2NO(g) What
is the partial pressure (atm) of NO in equilibrium with N2 and O2 that were
placed in a flask at initial pressures of 0.40 and 1.60 atm, respectively?
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