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The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N 2 and O 2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N 2 (g) + O 2 (g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N 2 and 0.100 mol L-’ ofO 2 , what were the equilibrium concentrations of all species?

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Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023

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Section
BuyFindarrow_forward

Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023
Chapter 12, Problem 12.42PAE
Textbook Problem
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The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained?

The following reaction establishes equilibrium at 2000 K:

N2(g) + O2(g) *2 2 NO
K = 4.1 X IO-4

If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?

Interpretation Introduction

Interpretation:

Equilibrium concentration are calculated by using ICE tables

Concept Introduction:

Equilibrium concentration are calculated by using ICE tables and using values of equilibrium constant K

To determine:

Equilibrium concentration of N2,O2andNO

Explanation of Solution

The equilibrium concentration of N2 and O2 are 0.1457 M and NO is 0.0086 M

Given:

K=3.6×103

Initial concentration of N2 is 0.15 mol

Initial concentration of O2 is 0.15 mol

Calculations:

Concentration= molesvolume=0.151.00=0.15M

Balanced reaction for the question is

N2(g)+O2(g)2NO(g)

ICE table:

I 0

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Chemistry for Engineering Students
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