benghazi

0.5 mol CCl4 is introduced into a 10.0L flask .what fraction of the total volume of flask is occupied by CCl4 molecules?

asked by jasmine
  1. all of it if it's a gas.
    If a liquid, then you need to look up the density of CCl4 (convert to g/L)
    find how many grams is .5 mol
    volume = mass/density
    divide that by 10.0L

    posted by Steve

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    0.5 mol CCl4 is introduced into a 10.0L flask.what fraction of the total volume of the flask is occupied by CCl4 molecules?
  2. Chemistry

    Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25°C. The vapor above this solutionis collected and condensed. Using the following data, determine the
  3. Chemisrty

    Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25°C. The vapor above this solutionis collected and condensed. Using the following data, determine the
  4. Chemistry

    Reposting with correct information..Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25°C. The vapor above this solutionis collected and condensed. Using the
  5. chemistry

    at 700 k the equilibrium constant for the reactions is Kp=0.76. Carbon tertrachrolide gas yields carbon solid and chlorine gas. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700K. A) what is the
  6. Chemistry

    Calculate the number of molecules in 3.11mol of CCL4 this is what I'm doing I got the molecular weight of CCL4 which is 181.88 Then I set it up like this 3.11 mol CCL4/ 181.88 mol CCL4 x 6.022E23 = 1.03E22 Am I right
  7. Chemistry

    Calculate the pressure that ccl4 will exert at 40 of 1.00 mol occupies 28.0 L, assuming that (a) CCl4 obeys the ideal-gas equation (b) CCl4 obeys the Van der Waals equation. (a) PV = nRT P = nRT / V (b) (P + n^2a/V^2)(V - nb) =
  8. College Chemistry

    If 69.3g of magnesium chloride were produced from a process with a known yield of 78.3%, find the mass of carbon tetrachloride in grams that was used. Equation: 2CCl4 + MgCrO4 -> 2COCl2 + CrO2Cl2 + MgCl2 I was able to solve it
  9. chemistry

    in a lab experiment to obtain the molar mass of a voltaile liquid, the following data is obtained: volume of flask=225ml mass of flask=77.834gms mass of flask+gas=78.416gms temperature=100 degrees celsius pressure=714 torr What is
  10. Chemistry

    Two gases are mixed in a 10.0L fixed volume flask: 8.0 L of O2 at 2.00 atm and 2.0 L of N2 at 3.00 atm. A) Calculate the partial pressure for each gas and the total pressure. I got ... PO2 = 1.60 atm PN2= 0.600 atm B) How much

More Similar Questions