×
Log in to StudySoup

Forgot password? Reset password here

Solved: Using the van der Waals EquationIf 10.00 mol of an

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780321910417 77

Solution for problem 2PE Chapter 10.15SE

Chemistry: The Central Science | 13th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 13th Edition

4 5 0 283 Reviews
14
0
Problem 2PE

Using the van der Waals Equation

If 10.00 mol of an ideal gas were confined to 22.41 L a: 0.0 aC. it would exert a pressure of

10.00        atm. Use the van der Waals equation and Table to estimate the pressure exerted by

1.000        mol of Ct2{g) in 22.41 L at 0.0 aC.

Table Van der Waals Constants for Gas Molecules

Substance        a L2@atm/mol2        b L moll

He                    0.0341                                0.02370

Ne                    0.211                                0.0171

Ar                    1.34                                0.0322

Kr                    2.32                                0.0303

Xe                    4.10                                0.0510

H2                    0.244                                0.0200

N2                    1.30                                0.0301

02                    1.38                                0.0318

F2                    1.06                                0.0200

CI2                    0.40                                0.0502

H20                    5.46                                0.0305

NH3                    4.17                                0.0371

CH4                    2.25                                0.0428

C02                    3.50                                0.0427

CCI4                    20.4                                0.1383

A sample of 1.000 mol of C02{g} is confined to a 3.000-L container at 0.000 aC. Calculate the pressure of the gas using (a) the ideal-gas equation and (b) the van der Waals equation.

Step-by-Step Solution:
Step 1 of 3
Step 2 of 3

Chapter 10.15SE, Problem 2PE is Solved
Step 3 of 3

Textbook: Chemistry: The Central Science
Edition: 13
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780321910417

Since the solution to 2PE from 10.15SE chapter was answered, more than 230 students have viewed the full step-by-step answer. This full solution covers the following key subjects: . This expansive textbook survival guide covers 305 chapters, and 6351 solutions. The answer to “Using the van der Waals EquationIf 10.00 mol of an ideal gas were confined to 22.41 L a: 0.0 aC. it would exert a pressure of10.00 atm. Use the van der Waals equation and Table to estimate the pressure exerted by1.000 mol of Ct2{g) in 22.41 L at 0.0 aC.Table Van der Waals Constants for Gas MoleculesSubstance a L2@atm/mol2 b L mollHe 0.0341 0.02370Ne 0.211 0.0171Ar 1.34 0.0322Kr 2.32 0.0303Xe 4.10 0.0510H2 0.244 0.0200N2 1.30 0.030102 1.38 0.0318F2 1.06 0.0200CI2 0.40 0.0502H20 5.46 0.0305NH3 4.17 0.0371CH4 2.25 0.0428C02 3.50 0.0427CCI4 20.4 0.1383A sample of 1.000 mol of C02{g} is confined to a 3.000-L container at 0.000 aC. Calculate the pressure of the gas using (a) the ideal-gas equation and (b) the van der Waals equation.” is broken down into a number of easy to follow steps, and 125 words. The full step-by-step solution to problem: 2PE from chapter: 10.15SE was answered by , our top Chemistry solution expert on 09/04/17, 09:30PM. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 13. Chemistry: The Central Science was written by and is associated to the ISBN: 9780321910417.

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

Solved: Using the van der Waals EquationIf 10.00 mol of an

×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide

Forgot password? Reset password here

Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide
Join with Email
Already have an account? Login here
Reset your password

I don't want to reset my password

Need an Account? Is not associated with an account
Sign up
We're here to help

Having trouble accessing your account? Let us help you, contact support at +1(510) 944-1054 or support@studysoup.com

Got it, thanks!
Password Reset Request Sent An email has been sent to the email address associated to your account. Follow the link in the email to reset your password. If you're having trouble finding our email please check your spam folder
Got it, thanks!
Already have an Account? Is already in use
Log in
Incorrect Password The password used to log in with this account is incorrect
Try Again

Forgot password? Reset it here