Chemistry

Two separate flasks are each filled with a gas at 25.0°C; the valve between them is opened and the gases are allowed to mix. What would be the final pressure in torr after mixing, if initially H2 is in the first flask (Volume = 4.000 L) at 271.8 torr and CCl4 is in the second flask (Volume = 1.000 L) at 372.7 torr?

"Key Concept:In gas mixtures we use Dalton's law, which states that the total pressure is the sum of the partial pressures of the individualt gases. In an ideal situation each gas should obey the ideal gas law. Each gas expands to the fill the two flasks. Use Boyle's law to predict the partial pressure of each after expansion. Add partial pressures."

  1. 👍 0
  2. 👎 0
  3. 👁 151
  1. This is the long way around but I would do it this way but let me call your attention to the fact that CCl4 is NOT a gas at 25 C. Unless you clear up that part of the problem you are wasting your time on the rest of this.
    Use PV = nRT for H2 and solve for n = number of mols.
    Use PV = nRT for CCl4 gas and solve for n.
    Add n H2 to n CCl4 = total n

    Then PV = nRT, substitute the total n and the total V and final T and solve for P

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    If there are 2L of H2 gas at .625 atm, and 1L of N2 gas at .200 atm isolated in two flasks, what are the final partial pressures of each, and the total pressure, after the valve between the two flasks has been opened and the gases

    asked by Lily on April 7, 2013
  2. physics

    Container with movable piston at top and valve near bottom is filled an ideal gas. Valve is opened and some gas slowly escapes. Valve is then closed and the piston appears to be at a lower position. System is in thermal

    asked by HELP, need ASAP on December 5, 2011
  3. Physics

    A cylinder with a valve at the bottom is filled with an ideal gas. The valve is now opened and some of the gas escapes slowly. The valve is then closed, after which the piston is observed to be at a lower position. Assume that the

    asked by Thomas Samuel Adams on November 21, 2010
  4. Chemistry

    Consider two flasks. What are the final partial pressure of H2 and N2 after the stopcock between the two flasks is opened? Assume the final volume is 3.00 L. What is the total pressure in torr? Flask 1: 2.00 L H2, 475 torr Flask

    asked by Victor on April 6, 2017
  5. physics

    An open-topped tank completely filled with water has a release valve near its bottom. The valve is 1.63 m below the water surface. Water is released from the valve to power a turbine, which generates electricity. The area of the

    asked by maria on October 26, 2011
  6. Physics

    A cylinder with a valve at the bottom is filled with an ideal gas. The valve is now opened and some of the gas escapes slowly. The valve is then closed, after which the piston is observed to be at a lower position. Assume that the

    asked by Carl on November 21, 2010
  7. physics

    An open-topped tank completely filled with water has a release valve near its bottom. The valve is 1.63 m below the water surface. Water is released from the valve to power a turbine, which generates electricity. The area of the

    asked by melisa on October 25, 2011
  8. physics

    An open-topped tank completely filled with water has a release valve near its bottom. The valve is h = 1.9 m below the water surface. Water is released from the valve to power a turbine, which generates electricity. The area of

    asked by Brandon on November 27, 2012
  9. Physics

    An open-topped tank completely filled with water has a release valve near its bottom. The valve is 1.75m below the water surface. Water is released from the valve to power a turbine, which generates electricity. The area of the

    asked by Santi on September 3, 2014
  10. chemistry

    Consider three one-liter flasks labeled A, B, and C filled with the gases NO, NO2, and N2O, respectively, each at STP. Which flask contains 1.0 mole of gas?

    asked by Anonymous on November 8, 2009

More Similar Questions