Question

Calculate the second Virial coefficient (B2) of Methane at 300 K from its van der Waals...

Calculate the second Virial coefficient (B2) of Methane at 300 K from its van der Waals constants: a0.2283 Pa m^6 mol^-2 and b = 0.0428x 10 ^-3 m^3 mol^-1. Calculate the compressibility factor at 300 K and 1 bar.

Homework Answers

Answer #1

Given conditions

Temperature T = 300 K

Pressure P = 1 bar

van der Waals constants

a = 0.2283 Pa.m6.mol-2

a = 0.2283 Pa * (1bar/10^5Pa) m6 * (1000L/m3)2 mol-2

a = 2.283 bar L2 mol-2

b = 0.0428 * 10^-3 m3.mol-1

b = 0.0428 * 10^-3 m3 * (1000L/m3) mol-1

b = 0.0428 L mol-1

First virial coefficient B1 = b - (a/RT)

= 0.0428 - (2.283/0.08314*300)

= - 0.0487 L/mol

Second virial coefficient B2 = b2

= ( 0.0428)2

= 1.83*10^-3 L2/mol2

Compressibility factor

Z = 1 + B1/V + B2/V2

Molar volume V = RT/P = 0.08314*300/1 = 24.942 L/mol

Z = 1 + (-0.0487/24.942) + (1.83*10^-3/24.9422)

Z = 1 - 0.0019525 + 2.9416*10^-6

Z = 0.99805

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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
The amount n = 2.00 mol of a van der Waals gas with a = 0.245...
The amount n = 2.00 mol of a van der Waals gas with a = 0.245 m6 Pa mol-2 occupies a volume of 0.840 L if the gas is at a temperature of 85.0 K and at a pressure of 2850 kPa. From this information, calculate the van der Waals constant b and the pressure p of this gas sample when it occupies a volume of 1.680 dm3 at T = 255 K.
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?
For ethane, C2H6, the van der Waals constants are a = 5.435x10−1 Pa.m6/mol−2 and b =...
For ethane, C2H6, the van der Waals constants are a = 5.435x10−1 Pa.m6/mol−2 and b = 6.51x10−5 m3/mol Calculate the pressure exerted by 1.0 mole of ethane and the compression factor Z: In a 20 L container at 300K as an ideal gas P = _______________ __________ Z = ___________ In a 20 L container at 300K as a van der Waals gas P = _______________ __________ Z = ___________ In an 100. mL container at 900 K as an...
Use both the van der Waals and the Redlich-Kwong equations to calculate the molar volume of...
Use both the van der Waals and the Redlich-Kwong equations to calculate the molar volume of CO at 213 K and 1036 bar. (Take a = 1.4734 dm6·bar·mol−2 and b = 0.039523 dm3·mol−1 for the van der Waals equation and A = 17.208 dm6·bar·mol−2·K1/2 and B = 0.027394 dm3·mol−1 for the Redlich-Kwong equation.) Calculate the molar volume under the same conditions using the ideal-gas equation. Answer in dm3·mol−1.
The amount 2.00 mol of a van der waals gas with a=0.245 m^6 Pa mol^-2 occupies...
The amount 2.00 mol of a van der waals gas with a=0.245 m^6 Pa mol^-2 occupies a volume of 0.840 L if the gas is at a temperature of 85k and at a pressure of 2850 kPa. From this information, calculate the van der waals constant b and pressure p of this sample when it occupies a volume of 1680 dm^3 at T=255k.
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
Derive an expression for the isothermal reversible expansion of a van der Waals gas. Account physically...
Derive an expression for the isothermal reversible expansion of a van der Waals gas. Account physically for the way in which the coefficients a and b appear in the expression. Using Maple, plot the expression along with that for an ideal gas. For the van der Waals gas, use a case first where a = 0 and b = 5.11 x 10-2 mol-1 and where a = 4.2 L2 atm mol-2 and b = 0. Take Vi = 1.0 L,...
A certain vapor obeys tge van der Waals equation with a=.56m^6Pa mole^-2. Its volume is 5.00x10-4m^3mole^-1...
A certain vapor obeys tge van der Waals equation with a=.56m^6Pa mole^-2. Its volume is 5.00x10-4m^3mole^-1 at 273 K and 3.0x10^6Pa. Calculate the value of the van der Waals constant b for this substance.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT