Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The equilibrium constant, Ke, for the reaction N204(8) 2 NO2(s) at 25 °C is 170. Suppose 13.9 g of N204 is placed in a 3.000-L flask at 25 °C. Calculate the following: a The amount of NO2 (mol) present at equilibrium is mol

The equilibrium constant, Ke, for the reaction N204(8) 2 NO2(s) at 25 °C is 170. Suppose 13.9 g of N204 is placed in a 3.000-L flask at 25 °C. Calculate the following: a The amount of NO2 (mol) present at equilibrium is mol

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
100%
The equilibrium constant, Ke, for the reaction N204(8) 2 NO2(s) at 25 °C is 170. Suppose 13.9 g of N204 is placed in a 3.000-L flask at 25 °C. Calculate the following: a The amount of NO2 (mol) present at equilibrium is mol
Transcribed Image Text:The equilibrium constant, Ke, for the reaction N204(8) 2 NO2(s) at 25 °C is 170. Suppose 13.9 g of N204 is placed in a 3.000-L flask at 25 °C. Calculate the following: a The amount of NO2 (mol) present at equilibrium is mol
Expert Solution
Step 1

Given chemical reaction,

N2O4 (g)⇌2 NO2 (g)

The equilibrium constant Kc = 170.

Mass of N2O4 = 13.9 g 

Volume of the flask = 3.000 L 

Molar mass of N2O4 = 92.011 g/mol 

Number of moles of N2O4 =

mass of N2O4 /Molar mass of N2O4 

Number of moles of N2O4 =

13.9 g/92.011 (g/mol)

Number of moles of N2O4 = 0.1511 mol 

Molarity of N2O4 = number of moles of N2O4 / Volume 

Molarity of N2O4 = 0.1511 mol/3.000 L

Molarity of N2O4 = 0.05037 M

steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Chemical Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS