Chemistry

A steel container of oxygen has a volume of 20.0 L at 22 C @35 atm. What is the volume @ STP? How many mol of oxygen are in the container?

  1. 👍
  2. 👎
  3. 👁
  1. i got the answer, 2.37L..and 28.90 mol.. but that doesnt seem right to me, wouldnt it be the other way around?

    P1V1/T1= 2.37 L
    n=PV/RT= 28.90 mol

    or should they be switched?

    1. 👍
    2. 👎
  2. I worked the problem and obtained 28.916 mol which rounds to 28.9 to three s.f. but 2.37 L isn't close.
    P1V1/T1 = 2.37. That is right; however, that isn't V2.
    You must equate 2.37 on the left to P2V2/T2 and plug in standard conditions. As Bob Pursley wrote,
    P1V1/T1 = P2V2/T2 and you have solved only half the equation.

    1. 👍
    2. 👎
  3. .0820 L?

    1. 👍
    2. 👎
  4. no.
    Post your work and I'll find what you are doing wrong.

    1. 👍
    2. 👎
  5. 2.37= 1atm*22.4L/273K

    1. 👍
    2. 👎
  6. Pray tell, what is the unknown. You have no unknown. In addition, what you have written is not an equality. 22.4/273 certainly isn't = 2.37.
    What is the problem asking for? I thought it wanted you to calculate the new volume at the new conditions? It asks, "What is the volume at STP?"

    1. 👍
    2. 👎
  7. Yes. i don't know why im having such a problem with this.
    35atm820.0L/295K= 2.37

    and the stp are, 273K, 1 atm, and 22.4 L

    1. 👍
    2. 👎
  8. No. STP conditions are 273 K and 1 atm p. Your problem, I think, is that you have somehow convinced yourself that the volume is 22.4 L since that is the volume of a mole of gas at STP. But you don't have a mole of gas. You have already figured moles at 28.9 or so and you have much more than 1 mole of gas. You must have much more than 22.4 if you have almost 30 moles of gas.
    p1 = 35 atm
    V1 = 20.0 L
    T1 = 273 + 22 = 295

    P2 = 1 atm
    V2 = unknown, solve for this.
    T2 = 273

    (35*20.0/295) = (1*V2/273)
    Solve for V2.
    (35*20.0/295) = (1*V2/273)

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chem.

    A sample of argon at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0. °C. What is the new pressure? 105 atm 45.5 atm 54.9 atm 23.8 atm 42.7 atm

  2. Chem H.W. Help!

    If You transfer a sample of a gas at 17 °C from a volume of 5.67 L and 1.10 atm to a container at 37 °C that has a pressure of 1.10 atm. What is the new volume of the gas?

  3. Chemistry

    At 298 K, the Henry\'s law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen.At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm? At 298 K, what is the solubility of oxygen in water exposed to

  4. sciencee

    1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?

  1. chemistry

    A sample of oxygen at room temperature occupies a volume of 500. L at 1.75 atm. What would be the volume of this gas at 2.50 atm at the same temperature?

  2. Chemistry

    The volume of a sample of oxygen is 300.0mL when the pressure is 1.00 atm and the temperature is 27.0 degrees C. At what temperature is the volume 1.00 L and the pressure 0.500 atm?

  3. Chem hw!

    1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?

  4. chem. mix of boyles and charles law

    The volume of a scuba tank is 10.0L.It containes a mixture of nitrogen and oxygen at 290.atm.what volume of this mixture could the tank supply to a diver at 2:40 atm?

  1. Chemistry

    The partial pressures of the gases in the container are monitored at constant temperature and recorded in the table below. At time t4, is the rate of the reverse reaction greater than, less than, or equal to the rate of the

  2. AP Chem

    Can someone please check these problems? 34. You fill a balloon with helium gas to a volume of 2.68 L at 23 degrees C and 789 mmHg. Now you release the balloon. What would be the volume of helium if its pressure changes to 632

  3. chemistry

    I need help setting up this problem: A 5.0 sample of O2 is in a container at STP. What volume is the container and how many molecules of O2 in the container and how many atoms of oxygen?

  4. chemistry

    can anyone help with this problem please..... Potassium chlorate decomposes according to the following equation: 2KClO3 (s) → 2KCl (s) + 3O2 (g). If a 3.00 g sample of KClO3 is decomposed and the oxygen is collected at 24.0 °C

You can view more similar questions or ask a new question.