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Year 12s: what will be the first way you research your future options? >>

Help in Chemistry2 15th may

Question is;
The equation for a reaction is
N2(g) + 3H2(g) *reversible* 2NH3(g)
A company wants to make 6.8 tonnes of ammonia
Calculate the mass of nitrogen needed.
Relative atomic masses (Ar): H=1 ; N=14
If you could explain this as clearly as possible.. You're a life saver
3 marks

(edited 9 years ago)

Mass=Mr x moles
6.8=mr(of ammonia which is 14+14+(1x6)=34) x moles
6.8/34=moles
Moles=0.2

Mr of nitrogen = 14+14=28
Substitute the Mr of nitrogen and moles for ammonia into mass=mr x moles
Mass=28 x 0.2=5.6 tonnes.

OP

Original post by Hippycnt

Mass=Mr x moles
6.8=mr(of ammonia which is 14+14+(1x6)=34) x moles
6.8/34=moles
Moles=0.2

Mr of nitrogen = 14+14=28
Substitute the Mr of nitrogen and moles for ammonia into mass=mr x moles
Mass=28 x 0.2=5.6 tonnes.

Thank you. but this was posted a year ago haha

http://filestore.aqa.org.uk/subjects/AQA-CH2HP-W-MS-JUN13.PDF

http://filestore.aqa.org.uk/subjects/AQA-CH2HP-W-MS-JUN13.PDF the marksceme

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