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At a certain temperature, K. - 0.914 for the reaction NO2(3) + NO(3) = N2O(3) + O2lg) A mixture was prepared containing 0.200 mol of each gas in a 5.00 L container. What will be the equilibrium concentrations of each gas? (NO2) M [NO] i M (N2O] M [02] M How will the concentrations then change if 0.0500 mol of NO2 is added to the equilibrium mixture? (NO2) M (NO] M (N2O] M [O2]

At a certain temperature, K. - 0.914 for the reaction NO2(3) + NO(3) = N2O(3) + O2lg) A mixture was prepared containing 0.200 mol of each gas in a 5.00 L container. What will be the equilibrium concentrations of each gas? (NO2) M [NO] i M (N2O] M [02] M How will the concentrations then change if 0.0500 mol of NO2 is added to the equilibrium mixture? (NO2) M (NO] M (N2O] M [O2]

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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 1RC: 1. Graphite and carbon dioxide are kept at constant volume at 1000 K until the reaction C(graphite)...
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At a certain temperature, K. = 0.914 for the reaction NO2(3) + NO(3): N2O(g) + O2(g) A mixture was prepared containing 0.200 mol of each gas in a 5.00 L container. What will be the equilibrium concentrations of each gas? [NO2] i M [NO] i M [N2O] M [02] M How will the concentrations then change if 0.0500 mol of NO2 is added to the equilibrium mixture? [NO2] M [NO] i [N2O] i M [02] M %3D ΣΣ
Transcribed Image Text:At a certain temperature, K. = 0.914 for the reaction NO2(3) + NO(3): N2O(g) + O2(g) A mixture was prepared containing 0.200 mol of each gas in a 5.00 L container. What will be the equilibrium concentrations of each gas? [NO2] i M [NO] i M [N2O] M [02] M How will the concentrations then change if 0.0500 mol of NO2 is added to the equilibrium mixture? [NO2] M [NO] i [N2O] i M [02] M %3D ΣΣ
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