DUE NOW. Please answer it correctly. To study the following reaction at 20 °C,NO(g) + NO₂(g) + H₂O(g) = 2HNO₂(g)a mixture of NO(g), NO₂(g), and H₂O(g) was prepared in a 10.0 L glass bulb.For NO, NO2, and HNO2, the initial concentrations were as follows: [NO] = [NO₂] = 4.83 x 10-3 M and [HNO₂] = 0.0 M. The initialpartial pressure of H₂O(g) was 15.9 torr. When equilibrium was reached, the HNO₂ concentration was 6.0 × 10-4 M.Calculate the equilibrium constant, Kc, for this reaction.Kc =MO

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To study the following reaction at 20 °C, NO(g) + NO₂(g) + H₂O(g) 2HNO₂(g) a mixture of NO(g), NO2(g), and H₂O(g) was prepared in a 10.0 L glass bulb. For NO, NO2, and HNO2, the initial concentrations were as follows: [NO] = [NO₂] = 4.83 × 10-3 M and [HNO₂] = 0.0 M. The initial partial pressure of H₂O(g) was 15.9 torr. When equilibrium was reached, the HNO₂ concentration was 6.0 × 10-4 M. Calculate the equilibrium constant, Kc, for this reaction. Kc = = i

To study the following reaction at 20 °C, NO(g) + NO₂(g) + H₂O(g) 2HNO₂(g) a mixture of NO(g), NO2(g), and H₂O(g) was prepared in a 10.0 L glass bulb. For NO, NO2, and HNO2, the initial concentrations were as follows: [NO] = [NO₂] = 4.83 × 10-3 M and [HNO₂] = 0.0 M. The initial partial pressure of H₂O(g) was 15.9 torr. When equilibrium was reached, the HNO₂ concentration was 6.0 × 10-4 M. Calculate the equilibrium constant, Kc, for this reaction. Kc = = i

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.3CE

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