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At 27 °C, Kp = 1.5 x 1018 for the reaction 3NO(g) N₂O(g) + NO₂(g) If 0.030 mol of NO were placed in a 1.00 L vessel and equilibrium were established, what would be the equilibrium concentrations of NO, N₂O, and NO2. [NO] = i 0.0006 [N₂O] = [NO₂] = 0.0098 0.0098 M M M

At 27 °C, Kp = 1.5 x 1018 for the reaction 3NO(g) N₂O(g) + NO₂(g) If 0.030 mol of NO were placed in a 1.00 L vessel and equilibrium were established, what would be the equilibrium concentrations of NO, N₂O, and NO2. [NO] = i 0.0006 [N₂O] = [NO₂] = 0.0098 0.0098 M M M

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.4: Using Equilibrium Constants In Calculations
Problem 15.5CYU: The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the...
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At 27 °C, K₂= 1.5 x 1018 for the reaction 3NO(g) N₂O(g) + NO₂(g) If 0.030 mol of NO were placed in a 1.00 L vessel and equilibrium were established, what would be the equilibrium concentrations of NO, N₂O, and NO2. [NO] = i 0.0006 [N₂O] = 0.0098 [NO₂] = 0.0098 M M M
Transcribed Image Text:At 27 °C, K₂= 1.5 x 1018 for the reaction 3NO(g) N₂O(g) + NO₂(g) If 0.030 mol of NO were placed in a 1.00 L vessel and equilibrium were established, what would be the equilibrium concentrations of NO, N₂O, and NO2. [NO] = i 0.0006 [N₂O] = 0.0098 [NO₂] = 0.0098 M M M
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