In a closed container at 1900 K nitrogen first reacts with oxygen to yield NO: N₂(g) + O₂(g) <---> 2NO(g) K_p = 2.3 x 10^-4 . However, NO(g) reacts in the second step with oxygen to produce NO₂(g): 2 NO(g) + O₂(g) <----> 2NO₂(g) K_p = 1.3 x 10^-4 . Calculate K_p and K_c at 1900 K for the following net reaction: N₂(g) + 2O₂(g) <----> 2NO₂(g)

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Keith LeannonLv2

11 Nov 2019

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Consider the air pollutants NO and NO2, contributors tophotochemical smog. Both can be formed by the reation betweenatmospheric nitrogen and oxygen. At 25 C,

N2(g)+O2(g)----2NO(g)K1=4.2E-31 (1)

N2(g)+2O2(g)----2NO2(g) K2=1.0E-18(2)

A) Wtire the equilibrium constant expression for the formationof two moles of NO at 25 C

B) CalculateK for the formation of one mole of NO at 25 C

C) Caluculate K for the decomposition of one mole of NO2 at 25C

D) Calculate K for the following reaction at 25 C

2NO(g)+O2(g)----2NO2(g)

Nitrogen dioxide can be formed fromnitrogen oxide and oxygen: <?xml:namespace prefix = o ns ="urn:schemas-microsoft-com:office:office" />

2NO (g) + O2 (g) <- -> 2NO2 (g)

At 1000K, the equilibrium constant Kc is1.20.

A system of NO,O2 and NO2 is analyzed andthe following concentrations are found: [O2]=1.25M [NO]=2.25M[NO2]=3.25M

Is the system at equilibrium with respect to the reaction above?If not, will the concentration of NO2 increase, decrease, or willthe system proceed to equilibrium?

When an 80.0 liter vessel containing 2.00 mole of NO2(g) was heatedto 200oC, 6% of the NO2(g) decomposed to NO(g) and O2(g). What isKc for the reaction at this temperature?

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(a) 3.1 x 10-6
(b) 8.3 x 10-3
(c) 2.7 x 10-2
(d) 2.1 x 10-4
(e) 6.2.x 10-5

I've been arriving at 9.05x10^-7 as my answer for Kc for somereason. The answer is noted as A. Can anybody please help?Thanks.