Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? 1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 1013 2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 1012 3) N2O4(g) → 2NO2(g) 80.3 0.111 None of the following 8.98 0.0123
Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? 1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 1013 2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 1012 3) N2O4(g) → 2NO2(g) 80.3 0.111 None of the following 8.98 0.0123
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 47QRT
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Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)?
1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 1013
2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 1012
3) N2O4(g) → 2NO2(g)
-
80.3
-
0.111
-
None of the following
-
8.98
-
0.0123
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