posted by .

Which of these gases would you expect to have the largest van der Waals constant a?

a. H2

b. HF

c. F2

  • Chemistry -


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. chemistry

    I have a problem that states: Find the pressure of a sample of carbon tetrachloride, CCl4 if 1.00 mol occupies 35.0L at 77.0 degress C (slightly above its normal boiling point). Assume that CCl4 obeys (a) the ideal gas law; (b) the …
  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. Chemsitry - Van Der Waals

    The constants "a" and "b" in the van der waals equation are "empirical coefficients". What exactly does that mean?
  7. Chemistry

    Use van der Waals’ equation to calculate the pressure exerted by 2.33 mol of ammo- nia at −3.7◦C in a 1.25 L container. The van der Waals’ constants for ammonia are a = 4.00 L2·atm/mol2 and b = 0.0400 L/mol. (The values …
  8. 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 …
  9. Chemistry

    Using the van der Waals equation, calculate the pressure (in atmospheres) exerted by 91.14 g of Cl2 at 91.11 °C in a 1.00 L container. The van der Waals constants for Cl2 are a = 6.490 L2*atm/mol2 and b = 0.05620 L/mol.
  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