Question

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 29.0 g...

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 29.0 g H2 at 20.0°C in a 1.00 L container.

Use the van der Waals equation and data in the hint to calculate the pressure exerted.

Now, calculate the pressure exerted, assuming that the gas behaves as an ideal gas.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 39.5 g...
At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 39.5 g H2 at 20.0°C in a 1.00 L container assuming in Part 1 non-ideal behavior and in Part 2 ideal behavior. 7th attempt Part 1 Use the van der Waals equation and data in the hint to calculate the pressure exerted. 862 atm Part 2 Now, calculate the pressue excerted assuming that the gas behaves as an ideal gas.
Determine the pressure in atm exerted by 1.00 mole of CH4 placed into a bulb with...
Determine the pressure in atm exerted by 1.00 mole of CH4 placed into a bulb with a volume of 244.6 mL at 25°C. Carry out two calculations: in the first calculation, assume that CH4 behaves as an ideal gas; in the second calculation, assume that CH4 behaves as a real gas and obeys the van der Waals equation Explain why the values of van der Waals constant b of noble gas elements increases with atomic number?
If 1.00 mol of argon is placed in a 0.500-L container at 29.0 ∘C , what...
If 1.00 mol of argon is placed in a 0.500-L container at 29.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.
Use the ideal gas equation and the Van der Waals equation to calculate the pressure exerted...
Use the ideal gas equation and the Van der Waals equation to calculate the pressure exerted by 1.00 mole of Argon at a volume of 1.31 L at 426 K. The van der Waals parameters a and b for Argon are 1.355 bar*dm6*mol-2 and 0.0320 dm3*mol-1, respectively. Is the attractive or repulsive portion of the potential dominant under these conditions?
Use the van der Waals equation and the ideal gas equation to calculate the pressure for...
Use the van der Waals equation and the ideal gas equation to calculate the pressure for 2.00 mol He gas in a 1.00 L container at 300.0 K. 1st attempt Part 1 (5 points) Ideal gas law pressure_____ atm Part 2 (5 points) Van der Waals pressure_____ atm
A. Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of...
A. Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature of 286.5 K . B. Use the ideal gas equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature of 286.5 K .
Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of Cl2...
Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature of 302.0 K . Use the ideal gas equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature of 302.0 K
Calculate the pressure exerted by 2 g of helium in a 300 mL container at −25°C...
Calculate the pressure exerted by 2 g of helium in a 300 mL container at −25°C using (a) the ideal gas law, (b) van der Waals equation. Suggest the reason for the difference between the non-ideal and ideal cases. Data: a = 3.46 ×10−3 Pa m6; b = 23.71×10−6 m3mol−1. (20 pts)
Use the van der Waals equation of state to calculate the pressure of 4.00 mol of...
Use the van der Waals equation of state to calculate the pressure of 4.00 mol of Xe at 483 K in a 4.20-L vessel. Van der Waals constants can be found here. Use the ideal gas equation to calculate the pressure under the same conditions.
Use the van der Waals equation of state to calculate the pressure of 2.90 mol of...
Use the van der Waals equation of state to calculate the pressure of 2.90 mol of CH4 at 457 K in a 4.50 L vessel. Van der Waals constants can be found here. P= ________ atm Use the ideal gas equation to calculate the pressure under the same conditions. P= ______ atm
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT