Chemistry

posted by .

Determine the density of methane (CH4) in g/L at 27.8oC and 1.1 atm.

  • Chemistry -

    The general gas formula of PV = nRT can be modified to
    P*molar mass = density*R*T

  • Chemistry -

    So I have gotten 2 different answers. I used V=nRT/P to get the volume. Which was 24.7. Then I used D=M/V and divided 16.042/24.7 to get .65g/L

    Is that right?

  • Chemistry -

    no. If you obtained two different answers why did you pick that one? You know something must be wrong. How did you get V = 24.7 L. If I plug those numbers into V =nRT/P I don't get that. But I do obtain a number that agrees with the formula I gave you.

  • Chemistry -

    V=nRT/P I used (1)(.0821)(300.8)/1=24.7

  • Chemistry -

    Two points.
    If T is to 4 places I would use R as 0.08205 although that won't make much difference.
    The other one makes more difference. P is 1.1 atm in the problem and not 1.

  • Chemistry -

    Yes, thank you for catching that. So with the corrections (except I kept R as .0821) I got (1)(.0821)(300.8)/1.1=22.45. Then 16.042/22.45=0.71g/L

    Is it now correct? I appreciate all your help!!!

  • Chemistry -

    Yes. If that 1.1 is 1.1 and not 1.10 atm, then 0.71 is right. If it is 1.10 you should have one more place in your answer.

  • Chemistry -

    THANK YOU!!!

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Determine the density of methane (CH4) in g/L at 24.7oC and 1.1 atm ideal gas eqn: P = (rho)RT, where: pressure: P = 1.1 atm specific gas constant: R, R = |R / M, where |R = 0.0821 L-atm / K-mol and, molecular weightCH4: M = 0.016 …
  2. Chemistry

    A mole of methane reacts with 64g of oxygen at 1 atm, 425 K. There are two ways in which methane can react with oxygen. It can either form water vapor and carbon dioxide or water vapor and carbon monoxide. After reaction the final …
  3. chem

    Determine the density of methane (CH4) in g/L at 21.9oC and 0.9 atm
  4. Chemistry

    There is a balloon filled with methane,CH4. If the mass of the methane is 68.34g, what is the volume of the balloon at 0.805 atm and a temperature of -10*C?
  5. chemistry

    A bacterial culture isolated from sewage produced 35.5 mL of methane, CH4, at 31oC and 1 atm. What is the volume of this methane at standard temperature and pressure?
  6. Chemistry

    Natural gas is almost entirely methane, CH4. What volume of natural gas at 20 C and 1.00 atm pressure is required to heat one quart of water from 20 C to 100 C?
  7. CHEMISTRY

    A mixture of methane and helium is placed in a 2.0 l flask at 27 degrees the partial pressure of methane is 0.72 ATM and the partial pressure of helium is 0.22 ATM . What is the mole fraction of ch4?
  8. chemistry

    Use Table 9.4 to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H2O and CO2. What Volume (in L) of methane is needed to produce 3287 kJ of heat for methane …
  9. Chemistry

    Compute the approximate density of methane, CH4, at 20oC and 5.00 atm. The molecular weight of methane is 16.0.
  10. Chemistry

    1. An empty balloon weighs 10.0 g and is filled to a volume of 20.0 L with CO gas. If the density of air at 25.0 °C and 1.00 atm is 1.17 g/L, will the balloon float?

More Similar Questions