Chemistry

posted by .

The van der Waals equation for real gases recognizes that

(A) the molecular atrractions between paritcles of a gas decreases the pressure exerted by the gas
(B) the non-zero volumes of gas particles effectively decrease the amount of "empty space" between them
(C) gas particles have non-zero volumes and interact with one another
(D) molar volumes of gases of different types are different
(E) All of the above statements are correct

would the correct answer be (E)?

  • Chemistry -

    (C) says it best; the others are vague or do not tell the whole story.

    (D) is not necessarily true, and whatever differences there between are between gases are very small

  • Chemistry -

    E is the answer, you are correct

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Gases - van der waals

    It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of volume in a container actually ocupied by Ar atoms …
  2. Chem

    In the van der waals equation, the constants a and b are: 1)used to correct for the finite volume of gas molecules and the attractive forces between molecules 2)equal to each other for any real gas 3)used to correct for the difference …
  3. Chemistry

    For Carbon dioxide, for a volume of 500 mL and temperature of 100 degrees celcius, calculate the pressures using the ideal gas law and the van der Waals equation. Explain any dicrepancies in the calculated values. Ideal Gas Equation: …
  4. Chemistry

    Decomposition reaction: CH2=CH2(g)---> CH4(g) + C (Graphite) If the decomposition begins at 10c and 40.0 atm with a gas density of .215 g/ml and the temp increases by 950K. (a) what is the final temperature of the confined gas (ignore …
  5. Chemistry

    According to the ideal gas law a 9.03 sample of oxygen gas in a 0.8112 container at 499k should exert a pressure of 456atm. By what % does the pressure calculated using van der waals equation differ from the ideal pressure?
  6. Chemistry

    Using the information on the table of van der Waals Constants of Some Common gases, calculate the pressure exerted by 4.37 moles of chlorine gas confined in a volume of 2.45 L at 38 degrees Celsius. Compare the pressure with that calculated …
  7. Chemistry

    Using the information on the table of van der Waals Constants of Some Common gases, calculate the pressure exerted by 4.37 moles of chlorine gas confined in a volume of 2.45 L at 38 degrees Celsius. Compare the pressure with that calculated …
  8. Chemistry

    Using the information on the table of van der Waals Constants of Some Common gases, calculate the pressure exerted by 4.37 moles of chlorine gas confined in a volume of 2.45 L at 38 degrees Celsius. Compare the pressure with that calculated …
  9. Chemistry

    The compound CH3F has van der Waals constants a = 5.009 atm•L2 /mol 2 and b = 0.0562 L/mol. Using both the ideal gas law and van der Waals’s equation, calculate the pressure expected for 25 mol of CH3F gas in a 5.00-L container …
  10. Chemistry

    Use the van der Waals equation of state to calculate the pressure of 3.60 mol of NH3 at 489 K in a 4.50-L vessel. Van der Waals constants can be found here. P= Use the ideal gas equation to calculate the pressure under the same conditions. …

More Similar Questions