Ask questions and get helpful responses.
Ask a New Question
  1. Questions

Chem Check

Can someone verify my answers please?

convert the folowing into a pressure reading expressed in torr

A. 1.25atm * 760torr/1.0atm = 950. torr

B. 2.48 x 10^-3 atm * 760torr/1.0atm = 1.88 torr

C. 4.75 x 10^4 atm* 760torr/1.0atm = 3.61 x 10^7 torr

D. 7.60 x 10^6atm * 760torr/1.0atm = 5.78 x 10^9 torr

Convert each of the folliwing into the unit specified

A. 125 mm Hg into atm
125mm * 1.0atm/760mm = .164 (or is it 0.16?)

B. 3.20 atm into Pa
3.20atm * 101.0kPa/1.0atm * 1000Pa/1kPa = 3.24 x 10^5 Pa

C. 5.38 kPa into torr

5.38kPa * 760torr/101.3kPa = 40.4 torr

Can you guys check for to see if I did this right?

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
Chopsticks

  1. I didn't check the math but the method looks ok for them. On B of the second set I think you made a typo when you wrote 101.0. I think you meant 101.3.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    DrBob222

  2. Oh yea thanks.

    A. 125 mm Hg into atm
    125mm * 1.0atm/760mm = .164 (or is it 0.16?)

    what would that answer be?

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    Chopsticks

  4. nvm i got it. its .164

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    Chopsticks

  5. 5.38kpa into mmHG

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    debie

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    CO+H2O CO2+H2 kp=0.0611 atm @2000K A reaction mixture initially contains a CO partial pressure of 1334 torr and H2O partial pressure of 1778 torr at 2000K. Whats the partial pressure of CO2 and H2? I got 381 torr for both, but its

  2. Chemistry

    An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has a partial pressure of 217.0 torr, 13.2 torr, and 13.2 torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 torr.

  3. Chemistry

    Determine the partial pressure of oxygen collected by water displacement if the water temperature is 20.0 ◦ C and the total pressure of the gases in the collection bottle is 760 torr. PH2O at 20.0 ◦ C is equal to 17.5 torr.

  4. Chemistry

    A tank of helium gas with a pressure of 210 torr at 0∘C is heated to give a pressure of 1100 torr .

  1. chemistry 105

    A 260-mL flask contains pure helium at a pressure of 743 torr. A second flask with a volume of 480 mL contains pure argon at a pressure of 715 torr. If the two flasks are connected through a stopcock and the stopcock is opened,

  2. chem

    In an experiment a mixture of oxygen and nitrogen gas is collected over water at 30'c and 700 torr pressure. What is the partial pressure of oxygen, if the partial pressure of nitrogen is 550 torr? (Vapour pressure of water at

  3. chemistry

    determine the vapor pressure of a solution at 55 degrees C that contains 34.2g NaCl in 375 mL of water. The vapor pressure of pure water at 55 degrees C is 118.1 torr. so Psolution=XsolventPsolvent I don't know why I'm not getting

  4. chemistry

    A gas mixture, has a total pressure of 300. Torr and consists of equal masses of Ne and Ar. What is the partial pressure of Ar, in Torr?

  1. Science

    Suppose that a sample of gas occupies 119 mL of volume at 25◦C and a pressure of 221 torr. What would be the volume if the pressure were changed to 647 torr at 25◦C? This is boyle's law right? p1v1 = p2v2 Since I'm looking for

  2. Chemistry

    Some hydrogen gas is collected over water at 20.0 Cel. and the levels inside the container is the same. The partial pressure of hydrogen is 742.5 torr. What is the barometric pressure as the time the gas was collected. My answer

  3. Chem

    A solution is made by mixing 50.0 g C3H6O and 50.0 g of CH3OH. What is the vapor pressure of this solution at 25 degrees C? What is the composition of the vapor expressed as a mole fraction? Assume ideal solution and gas behavior.

  4. Chemistry

    A sample of gas is collected over water at a temperature of 45.0 oC when barometric pressure reading is 742.0 torr. What is the partial pressure of the dry gas?

Still need help? You can ask a new question.