(b) Consider the reversible decomposition of nitrogen monoxide to form nitrogen dioxide and dinitrogen monoxide. (i) If 5.38 mol of nitrogen dioxide and 7.47 mol of dinitrogen monoxide were placed in a 1 L vessel at 220 °C and 2.64 mol of nitrogen dioxide were present at equilibrium, calculate the moles of nitrogen monoxide that were initially placed in the reaction vessel, given that the pressure equilibrium constant for the reaction is 3.21 x 10“ atm". (ii) If this exothermic decomposition reaction was done at 785 °C, what would be the impact on the concentration of each chemical species as well as the equilibrium constant for the reaction?

(b) Consider the reversible decomposition of nitrogen monoxide to form nitrogen dioxide and dinitrogen monoxide. (i) If 5.38 mol of nitrogen dioxide and 7.47 mol of dinitrogen monoxide were placed in a 1 L vessel at 220 °C and 2.64 mol of nitrogen dioxide were present at equilibrium, calculate the moles of nitrogen monoxide that were initially placed in the reaction vessel, given that the pressure equilibrium constant for the reaction is 3.21 x 10“ atm". (ii) If this exothermic decomposition reaction was done at 785 °C, what would be the impact on the concentration of each chemical species as well as the equilibrium constant for the reaction?

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 92QRT

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