answer

watching

views

pucehamster19Lv1

6 Oct 2020

You want to store 165 g of CO₂ gas in a 12.5-L tank at room temperature (25 °C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO₂, a = 3.59 atm•L²/mol² and b = 0.0427 L/mol.)

answer

watching

374

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Patrick SuarezLv10

18 Nov 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

1) A 10.60 mol sample of argon gas is maintained in a 0.8466 L container at 298.6 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L²atm/mol² and b = 3.219Ã10^-2 L/mol.

A: ______ atm

2) According to the ideal gas law, a 1.007 mol sample of argon gas in a 1.337 L container at 272.3 K should exert a pressure of 16.83 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Ar gas, a = 1.345 L²atm/mol² and b = 3.219Ã10^-2L/mol.

Hint: % difference = 100Ã(P _ideal - P_{van der Waals}) / P _ideal

A: ________% â

1 . Calculate the pressure (in atm) of 16.80 mol ofCO₂ gas in a 3.00 L vessel at 153 K with:

(a) the ideal gas law

(b) the Van der Waals equation (a= 3.592L²â¢atm/mol² and b= 0.0427 L/mol forCO₂)

2. What volumeof H₂ (at 25^oC and 1.00 atm ) can be producedby reaction of 161 g Fe and 202 g of HCl? (Atomic weights: Fe =55.85, Cl = 35.45, H = 1.008).

Fe + 2 HCl FeCl₂ +H₂

***Make sure you pay attention to significant figuresand give proper units with your answers

amaranthtrout522

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

You want to store 165 g of CO₂ gas in a 12.5-L tank at room temperature (25 °C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO₂, a = 3.59 atm•L²/mol² and b = 0.0427 L/mol.)

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25 °C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm•L2/mol2 and b = 0.0427 L/mol.)

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

You want to store 165 g of CO₂ gas in a 12.5-L tank at room temperature (25 °C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO₂, a = 3.59 atm•L²/mol² and b = 0.0427 L/mol.)