Subjects

Sections | |||
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Pressure Units | 10 mins | 0 completed | Learn |

Manometer | 10 mins | 0 completed | Learn Summary |

Partial Pressure | 11 mins | 0 completed | Learn Summary |

The Ideal Gas Law | 47 mins | 0 completed | Learn Summary |

Standard Temperature and Pressure | 19 mins | 0 completed | Learn |

Effusion | 8 mins | 0 completed | Learn Summary |

Root Mean Square Speed | 11 mins | 0 completed | Learn Summary |

Kinetic Molecular Theory | 9 mins | 0 completed | Learn |

Van der Waals Equation | 22 mins | 0 completed | Learn |

Velocity Distribution | 7 mins | 0 completed | Learn |

End of Chapter 5 Problems | 74 mins | 0 completed | Learn |

Additional Practice |
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Chemistry Gas Laws |

Ideal Gas Law Density |

Ideal Gas Law Molar Mass |

Gas Stoichiometry |

Collecting Gas Over Water |

Kinetic Energy of Gases |

Additional Guides |
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Ideal Gas Law |

Boyle's Law |

Combined Gas Law |

Solution: 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 diff

Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000 mol of Cl_{2} 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 and the ideal gas e...

Which gas molecule do you expect to be the largest...

Which gas would you expect to have the largest val...

The constant a in the Van der Waal’s equation corr...

Assuming that the van der Waals equation predictio...

Assuming that the van der Waals equation predictio...

Assuming that the van der Waals equation predictio...

Assuming that the van der Waals equation predictio...

In Sample Exercise 10.16 in the textbook, we found...

Calculate the pressure exerted by 1.00 mol of Ne i...

Calculate the pressure exerted by 1.00 mol of H2 i...

Calculate the pressure exerted by 1.00 mol of CH4 ...

Calculate the pressure exerted by 1.00 mol of CO2 ...

In Sample Exercise 10.16 in the textbook, we found...

Calculate the pressure that CCl4 will exert at 41 ...

Use the van der Waals equation and the ideal gas e...

The graph below shows the change in pressure as th...

Calculate the pressure of a 2.975-mol sample of N2...

Use the van der Waals equation of state to calcula...

Assuming that the van der Waals equation predictio...

The table below shows that the van der Waals b par...

Which statement(s) concerning the van der Waals co...

Describe the factors responsible for the deviation...

For which of the following gases should the correc...

A 0.245-L flask contains 0.467 mol CO2 at 159 °C. ...

For each of the following, which shows the greater...

For each of the following, which shows the greater...

For each of the following, which shows the greater...

For each of the following, which shows the greater...

In the following table shows that the van der Waal...

Large amounts of nitrogen gas are used in the manu...

Calculate the pressure exerted by 0.5000 mole of N...

Calculate the pressure exerted by 0.5000 mole of N...

Calculate the pressure exerted by 1.00 mol of He i...

Many water treatment plants use chlorine gas to ki...

Use the van der Waals equation to calculate the pr...

A 0.245-L flask contains 0.467 mol CO2 at 159 °C. ...

Large amounts of nitrogen gas are used in the manu...

Ammonia is essential to so many industries that, o...

Calculate the pressure exerted by 0.5000 mole of N...

Calculate the pressure exerted by 0.5000 mole of N...

Chlorine is produced from sodium chloride by the e...

A slight deviation from ideal behavior exists even...

The ideal gas law tends to become inaccurate when ...

Use the van der Waal's equation to calculate the p...

Calculate the pressure (atm) that CCl4 will exert ...Calculate the pressure in bar of 8.5 mol of ethano...At high pressures, real gases do not behave ideall...Use the van der Waals equation to calculate the pr...Use the van der Waals equation of state to calcula...Use the van der Waals equation of state to calcula...Use the van der Waals equation of state to calcula...According to the ideal gas law, a 9.847 mol sample...Part B If 1.00 mol of argon is placed in a 0.500-L...15.0 moles of gas are in a 8.00 L tank at 22.2°C. ...At high pressures, real gases do not behave ideall...

It turns out that the van der Waals constant b equ...

The graph below shows the change in pressure as th...

To study a key fuel-cell reaction, a chemical engi...

Based on their respective van der Waals constants,...

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