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# Moles, Haber Process Question GCSE chemistry watch

1. 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!
2. 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
3. (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!
4. 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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