Post a New Question

Chemistry

posted by .

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 for a and b have been rounded off to simplify the arithmetic.)
1. 22.9782 atm 2. 30.6376 atm 3. 40.8502 atm 4. 15.3188 atm 5. 61.2752 atm

  • Chemistry -

    Isn't this just a matter of substituting the numbers into the van der waals equation? What's the problem?

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

    Water has a van der Waals constants of a = 5.464 L·atm/mol2 and b = 0.03049 L/mol. What is the pressure of 5.20 moles of water vapor in a 1.10 L container at 100.0°C?
  4. chm

    calculate the van dar waals coorectionj terms to pressure and volume for Cl2 at STP. The values of the van der waals constant a and b are 6.49L2-atm/mol2 and 0.056L/mol, respectively, for Cl2. At STP, which is the major cause of deviation …
  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

    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 …
  8. Chemistry

    Calculate the pressure exerted by a 14.6 mol NH3g in a 3.2 L container at -15.0 celcius using the Van der Waals equation.
  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

Post a New Question