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anonymous

  • one year ago

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 degrees C into a 7.0 L flask. The total pressure in the flask is ____ atm. Assume the initial pressure in the flask was 0.00 atm. Please show and explain steps please! I believe this involves partial pressure

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  1. anonymous
    • one year ago
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    Please help!

  2. Rushwr
    • one year ago
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    Okai it's like this, We can see both the gases have an end volume 7L right? Use the below equation for each gas separately using the final volume as 7L . Since the temperature is constant we can use \[P _{1}V _{1} =P _{2}V _{2}\] P1 and V1 are initial pressure and volume. P2 and V2 are the final pressure and final volume .

  3. Rushwr
    • one year ago
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    first apply that for H2 gas P1 = 3.5atm V1 = 2L P2 = is unknown , the thing we are going to find V2 = 7L . Because gases take the volume of the container. Now we can find the partial pressure given from H2 to the total pressure. Do the same thing for N2 and get the pressure from that Then use Dalton's law total pressure = partial pressures of the gases \[P = P _{H _{2}} + P _{N _{2}}\]

  4. Rushwr
    • one year ago
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    Did u get it ? @makenzie_paige

  5. anonymous
    • one year ago
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    1.56?

  6. Rushwr
    • one year ago
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    wait I didn't take the answer ! I'll quickly calculate !

  7. anonymous
    • one year ago
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    Thank you!

  8. Rushwr
    • one year ago
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    yep correct !!! :)

  9. anonymous
    • one year ago
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    Yay! Thank you so much!

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