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Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas.

Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N,O4(g)=2 NO,(g) Three experiments were run starting with different initial amounts of N,O4(g) ([N204]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 N,04 at equilibrium. Be sure to round to the correct number of significant figures. Exp N,04lo NO, N,0,1 NO,] / [N,04 2 NO,] / N,041 NO,12 / N,04] 3.5 2.85 2.1 12 3.0 2.56 1.7 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. v 2. The ratio ([NO] / [N2O4]) is equal to a constant value. v3. The ratio (2 [NO,]/ [N,041) is equal to a constant value. 4. The ratio ([NO2] / [N204]) is equal to a constant value. v5. Each experiment reached a different set of equilibrium concentrations. Previous Nex
Transcribed Image Text:Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N,O4(g)=2 NO,(g) Three experiments were run starting with different initial amounts of N,O4(g) ([N204]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 N,04 at equilibrium. Be sure to round to the correct number of significant figures. Exp N,04lo NO, N,0,1 NO,] / [N,04 2 NO,] / N,041 NO,12 / N,04] 3.5 2.85 2.1 12 3.0 2.56 1.7 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. v 2. The ratio ([NO] / [N2O4]) is equal to a constant value. v3. The ratio (2 [NO,]/ [N,041) is equal to a constant value. 4. The ratio ([NO2] / [N204]) is equal to a constant value. v5. Each experiment reached a different set of equilibrium concentrations. Previous Nex
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