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# Use the equilibrium constants for the following reactions at 700 0C 2SO2(g) + O2(g) 2SO3(g) K1 = 4.8 2NO(g) + O2(g) 2NO2(g) K2 = 16 to determine the equilibrium constant for the following reaction. SO3(g) + NO(g) SO2(g) + NO2(g) A. 0.30
B. 0.55
C. 0.85
D. 1.8
E. 3.3

This question is part of CHEM 2425
Asked by Ochiengj, Last updated: May 11, 2020

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Ochiengj

1.8

Solving: K1 = SO3(g)2 / SO2(g)2 O2(g) K2 = NO2(g)2/ NO(g)2 O2(g) K = SO2(g) NO2(g) / NO(g) SO3(g) = (SO2(g)2 O2(g)/ SO3(g)2 ) � (SO3(g) NO(g)/ SO2(g) NO 2(g)) � ( NO2(g)2/ NO(g)2 O2(g)) = 1/ K1 � 1/K � K2 K2 = K2 / K1 =16 /4.8 = 3.33 K = 1.8    Search for Google images Select a recommended image
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