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Moles, Haber Process Question GCSE chemistry watch

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    Hi

    So the question is

    Assuming 100% conversion of nitrogen gas and hydrogen gas into ammonia, calculate the maximum volume of ammonia that could be produced from 1200dm3 of hydrogen, measured at room temp and pressure.

    I have absolutely no idea how to answer this, so I'd really appreciate if someone talked me through it.

    Thank you!
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    The Haber process equation is
    N2(g) + 3H2(g) Equilibrium symbol 2NH3(g)


    1 mole of gas at room temperature and pressure occupies 24dm3
    therefore 1200/24=50
    50 mole of hydrogen
    =(50/3 )*2 moles of nitrogen due to the ratio.
    =33.33 mole of ammonia
    = 33.33*24 (1 mole of gas at room temperature and pressure occupies 24dm3)
    =800 dm3


    let me know if you have any questions
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    (Original post by Amrak)
    The Haber process equation is
    N2(g) + 3H2(g) Equilibrium symbol 2NH3(g)


    1 mole of gas at room temperature and pressure occupies 24dm3
    therefore 1200/24=50
    50 mole of hydrogen
    =(50/3 )*2 moles of nitrogen due to the ratio.
    =33.33 mole of ammonia
    = 33.33*24 (1 mole of gas at room temperature and pressure occupies 24dm3)
    =800 dm3


    let me know if you have any questions
    Thats perfect, thank you!
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    You don"t evwn need to go through the process of calculating the number of moles of gas you start or finish with, if you appreciate that a mole of any gas will have the same volume at any fixed conditions (fixed temp and pressure).

    From the equation you can get as much as 2/3 as much ammonia as you have hydrogen (in moles). As the conditions don"t change yoi can deduce that ou can ger 2/3 as much volume as you had of hydrogen.
 
 
 
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