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4 February, 05:20

What is the mass of 23450 L of hydrogen gas at STP

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Answers (1)
  1. 4 February, 08:23
    0
    Remember that in this case pressure is equal to 1.00 atm and temperature is equal to 273.15K. So,

    P

    V

    =

    n

    R

    T



    n

    =

    P

    V

    R

    T

    =

    1.00

    a

    t

    m



    7.0

    L

    0.082

    a

    t

    m



    L

    m

    o

    l



    K



    273.15

    K

    =

    0.31

    Since we know hydrogen's molar mass (

    2.0

    g

    m

    o

    l

    ), we can determine the mass

    m

    H

    2

    =

    n



    m

    o

    l

    a

    r

    .

    m

    a

    s

    s

    =

    0.31

    m

    o

    l

    e

    s



    2.0

    g

    m

    o

    l

    =

    0.62

    g

    If indeed you are dealing with STP, remember that, under these conditions, 1 mole of any ideal gas occupies

    22.4

    L

    . So,

    n

    =

    V

    V

    m

    o

    l

    a

    r

    =

    7.0

    L

    22.4

    L

    =

    0.31

    moles

    And, once again,

    m

    =

    0.31



    2.0

    =

    0.6
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