Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol of NO . The...

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Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol ofNO . The following reaction becomes possible: N2g+O2g =2NOg Theequilibrium constant K for this reaction is 0.469 at thetemperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to one decimal place.

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4.2 Ratings (609 Votes)

Â Â Â Â Â Â Â Â Â Â Â Â N2(g)+O2(g )---------->2NOg

IÂ Â Â Â Â Â Â Â x Â Â Â Â Â Â Â 2 0

C -1.6 Â Â -1.6 Â Â 1.6

E Â Â x-1.6 0.4 1.6

Â Â Kc = [NO]²/[N2][O2]

0.469 = (1.6)²/(x-1.6)(0.4)

0.469(x-1.6)(0.4) = 2.56

Â Â Â Â Â Â Â Â Â 0.1876x-0.30016Â Â Â = 2.56

Â Â Â Â Â Â Â Â 0.1876xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 2.56+0.30016

Â Â Â Â Â Â Â 0.1876xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 2.86016

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â =2.86016/0.1876Â Â Â = 15.246 moles

[N2]Â Â = x-1.6 = 15.246-1.6 = 13.646moles

molarity of N2 = 13.646/0.25Â Â =54. 584M

Â Â Â Â Â Â Â

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Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol of NO . The...

Free

90.2K

Verified Solution

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Chemistry

Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol ofNO . The following reaction becomes possible: N2g+O2g =2NOg Theequilibrium constant K for this reaction is 0.469 at thetemperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to one decimal place.

Answer & Explanation Solved by verified expert

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