Practice: Which gaseous compound is expected to have the largest value for the Van der Waals constant b?

a) O_{2}

b) CH_{3}CH_{3}

c) HBr

d) S_{8}

e) Ne

Subjects

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Pressure Units | 6 mins | 0 completed | Learn |

The Ideal Gas Law | 19 mins | 0 completed | Learn Summary |

The Ideal Gas Law Derivations | 6 mins | 0 completed | Learn |

The Ideal Gas Law Applications | 7 mins | 0 completed | Learn |

Chemistry Gas Laws | 16 mins | 0 completed | Learn |

Chemistry Gas Laws: Combined Gas Law | 12 mins | 0 completed | Learn |

Mole Fraction | 6 mins | 0 completed | Learn |

Partial Pressure | 19 mins | 0 completed | Learn Summary |

The Ideal Gas Law: Molar Mass | 19 mins | 0 completed | Learn |

The Ideal Gas Law: Density | 16 mins | 0 completed | Learn Summary |

Gas Stoichiometry | 7 mins | 0 completed | Learn |

Standard Temperature and Pressure | 14 mins | 0 completed | Learn |

Effusion | 13 mins | 0 completed | Learn Summary |

Root Mean Square Speed | 9 mins | 0 completed | Learn Summary |

Kinetic Energy of Gases | 5 mins | 0 completed | Learn |

Maxwell-Boltzmann Distribution | 8 mins | 0 completed | Learn |

Velocity Distributions | 5 mins | 0 completed | Learn |

Kinetic Molecular Theory | 7 mins | 0 completed | Learn |

Van der Waals Equation | 9 mins | 0 completed | Learn |

Additional Practice |
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Manometer |

Collecting Gas Over Water |

Additional Guides |
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Boyle's Law (IGNORE) |

Charles Law (IGNORE) |

Ideal Gas Law (IGNORE) |

The **Van der Waals Equation** is used when dealing with real, non-ideal gases.

Example #1: Using the Van der Waals equation, determine the pressure of 20.0 g oxygen gas in 250 mL graduated flask when the temperature is 50 ºC.

Practice: Which gaseous compound is expected to have the largest value for the Van der Waals constant b?

a) O_{2}

b) CH_{3}CH_{3}

c) HBr

d) S_{8}

e) Ne

0 of 4 completed

Which gas would you expect to have the largest value for the van der Waals constant “a”?
1. Ne
2. CH4
3. He
4. NH3

The constant a in the Van der Waal’s equation corrects for ________and is important at ________.
a. intermolecular attraction, high temperature
b. intermolecular attraction, low temperature
c. lower than average energy of molecules, low temperature
d. volume of molecules, low pressure
e. volume of molecules, high pressure

Which gas molecule do you expect to be the largest? (a and b are Van der Waals constants.)
1. Butane
2. Acetonitrile
3. Freon

Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000 mol of Cl2 in a volume of 5.000 L. at a temperature of 273.0 K. Explain why the two values are different.

Use the van der Waals equation of state to calculate the pressure of 2.70 mol of Xe at 473 K in a 5.50-L vessel. Van der Waals constants can be found below.P= ______________ atmUse the ideal gas equation to calculate the pressure under the same conditions.P=_______________atm

The graph below shows the change in pressure as the temperature
increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2.Use the van der Waals constants in the table below to
match the labels in the plot (A, B, and C) with the respective
gases (CO2, N2, and Cl2).

Use the van der Waal's equation to calculate the pressure (in atm) exerted by 1.00 mol of chlorine gas confined to a volume of 2.00 L at 273K. The value of a = 6.49 L2 atm mol-2, and that of b = 0.0562 L mol-1 for chlorine gas.a) no given answer is closeb) 9.9c) 4.12d) 1.54e) 3.73

Part B If 1.00 mol of argon is placed in a 0.500-L container at 30.0°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 = 0.03219 L/mol.Express your answer to two significant figures and include the appropriate units.

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