posted by .

Nitrogen and hydrogen, with volumes of 12.0 L each, are injected into a sealed rigid reaction chamber containing a catalyst. The pressure of the chamber is 8.00 atmospheres and at a known temperature. The reaction is allowed to proceed to completion while being maintained at a constant temperature. How many liters of each gas is present after the reaction occurs?

What is the partial pressure of each gas after the reaction goes to completion?

Which of the following statements about an ideal gas is incorrect?

A. There is no interaction between the particles of gas.­
B. The gas particles occupy negligible volume.
C. The "free volume" is the same as the volume of the container.
D. Gases behave ideally under conditions of standard temperature and pressure.
E. Gases under conditions of low pressure and high temperature are closest to "ideal."

I need these answered ASAP (w/i 24 hrs)!!!!

Please answer quickly, even if you only know one of the question's answers.

Thanks in advance!! :)

  • Chemistry -

    You need a Keq (Kc or Kp) for the reaction.

  • Chemistry -

    I would look at D as being the untrue statement.

  • Chemistry -

    The problem in 1 says that it proceeds to "completion" which means to me that we don't worry about the Kc or Kp.
    N2 + 3H2 ==> 2NH3. Since both reactants are given we know it is a limiting reagent problem. This is a gas problem; therefore, we are allowed to use L directly as moles.
    L NH3 formed if N2 is limiting = 12*2 = 24L.
    L NH3 formed if H2 is limiting = 12*(2 moles NH3/3 moles H2) = 12(2/3 = 8 L.
    The smaller value is always the correct one to chose; therefore, we will have 8 L NH3 formed and 12 L H2 used and H2 is the limiting reagent.
    How much H2 used? All of it; therefore, there is zero H2 remaining.
    How much N2 remains? How much is used.
    N2 used 8L NH3 x (1 mole N2/2 moles NH3) = 4 moles N2 used. Subtract from initial to find that remaining.

  • Chemistry -

    Thanks for question 1. So what would the partial pressure be for the gases?

  • Chemistry -

    I got 2.67 and 5.33 (b/c I did 3x = 8 atm (2x for NH3 and x for N2). Is that on the right track?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions


    A 8.90-g sample of ethane, C2H6, is mixed with 18.8 atm of O2 (an excess) in a 1.50 L combustion chamber at 130.0°C. The combustion reaction to CO2 and H2O is initiated and the vessel is cooled back to 130.0°C. What is the final …
  2. Chemistry

    Which of the following is the BEST explanation for why a catalyst speeds up a reaction?
  3. physics

    Some hydrogen gas is enclosed within a chamber being held at 200 whose volume is 0.0250 . Initially, the pressure in the gas is (14.8 ). The chamber is removed from the heat source and allowed to cool until the pressure in the gas …
  4. Chemistry

    A chemist is preparing to carry out a reaction at high pressure that requires 36.0 mol of hydrogen gas. The chemist pumps the hydrogen into a 15.5L rigid steel container at 25 degrees Celcius. To what pressure (in atmospheres) must …
  5. physics

    a 10.0 cm cylindrical chamber has a 5.0cm diameter piston attached to one end. The piston is connected to an ideal spring with a spring constant of 10.0N/cm. Initially, the spring is not compressed but is latched in place so that it …
  6. Gen Chm II

    Determine the pressure-based Keq for the reaction: 2SO2(g) + O2(g)<--->2SO3(g) given that 1.00×10−2 moles of SO2 and 2.00×10−2 moles of O2 were initially placed in a 2.00 L reaction chamber. The chamber contained …
  7. Chemistry

    A mouse is placed in a sealed chamber with air at 755.0 torr. This chamber is equipped with enough solid KOH to absorb any CO2 and H2O produced by the mouse. The gas volume in this chamber is measured to be exactly 1.70 L, the temperature …
  8. Chemistry

    Could you show me where to start on solving this equation?
  9. Chemistry

    Could you show me where to start on solving this equation?
  10. Chemistry

    Could you show me where to start on solving this equation?

More Similar Questions