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    Hey, Kinda stuck on this question

    Given a 4-gram sample of each H2(g) and He(g), each in separate containers, which of the following statements is true? (Assume STP)
    a) The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain 6.02 x 10^23 molecules
    b) The sample of hydrogen gas will occupy 22.4 liters and the sample of helium will contain 3.02 x 10^23 molecules
    c) The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain 1.202 x 10^24 molecules
    d) The sample of helium will occupy 44.8 liters and the sample of hydrogen gas will contain 6.02 x 10623 molecules
    e) None of the above statements is correct

    After calculating there are 2 moles of Hydrogen and 1 mole of He. Since 1 mole of gas occupies 22.4 then 2 moles would occupy 44.8 L and will also have 1.202 x10^24 molecules. The answer is saying A and I just dont understand why.

    Thanks
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    You're misreading.

    As you said, you have 2 mol of H2 and 1 mol of He.

    The Q doesn't ask you how many particles of H2 you have.
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    Hmm ok, but would it not have 1.202 x 10^24 molecules? i.e.Why is it answer A but not Answer C?
    (Original post by Pigster)
    You're misreading.

    As you said, you have 2 mol of H2 and 1 mol of He.

    The Q doesn't ask you how many particles of H2 you have.
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    Avagadros constant: 6.02x10^23. The number of particles in ONE mole
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    Yeah so 1 mole of H2 contains 6.02x10^23. In the question it has 2 moles of H2 so would'nt it just be double?
    (Original post by BDunlop)
    Avagadros constant: 6.02x10^23. The number of particles in ONE mole
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    (Original post by ChemBoy1)
    Yeah so 1 mole of H2 contains 6.02x10^23. In the question it has 2 moles of H2 so would'nt it just be double?
    You're not reading a) properly
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    Thank you! Wow I really made a mess of that
    (Original post by BDunlop)
    You're not reading a) properly
 
 
 
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