Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N204(9) =2 NO2(g) Three experiments were run starting with different initial amounts of N,04(g) ([N,04]o in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO, and N204 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N204lo [NO2] [N204] [NO2] / [N204] 2 [NO2] / [N204] [NO2]² / [N204] 1 3.7 2.92 2.2 2 2.8 2.49 1.6 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N204. v2. The ratio ([NO2] / [N2O4]) is equal to a constant value. v3. The ratio (2 [NO2] / [N2O4]) is equal to a constant value. v4. The ratio ([NO2]² / [N2O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.

Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N204(9) =2 NO2(g) Three experiments were run starting with different initial amounts of N,04(g) ([N,04]o in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO, and N204 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N204lo [NO2] [N204] [NO2] / [N204] 2 [NO2] / [N204] [NO2]² / [N204] 1 3.7 2.92 2.2 2 2.8 2.49 1.6 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N204. v2. The ratio ([NO2] / [N2O4]) is equal to a constant value. v3. The ratio (2 [NO2] / [N2O4]) is equal to a constant value. v4. The ratio ([NO2]² / [N2O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.

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 101QRT: Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three...

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