a.f.x.d
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Ammonia is manufactured from hydrogen and nitrogen in the Haber process.

3H2(g) + N2(g) -----> 2NH3(g)

If 60 tonnes of hydrogen produces 80 tonnes of ammonia, what is the percentage yield in the reaction?



The answer is 80/340 x 100% but I don't know-how. can someone explain?
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EierVonSatan
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(Original post by a.f.x.d)
Ammonia is manufactured from hydrogen and nitrogen in the Haber process.

3H2(g) + N2(g) -----> 2NH3(g)

If 60 tonnes of hydrogen produces 80 tonnes of ammonia, what is the percentage yield in the reaction?



The answer is 80/340 x 100% but I don't know-how. can someone explain?
It's using the formula (actual/max) x 100 where 80 tonnes is the actual mass produced and the 340 was the maximum mass possible.
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a.f.x.d
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(Original post by EierVonSatan)
It's using the formula (actual/max) x 100 where 80 tonnes is the actual mass produced and the 340 was the maximum mass possible.
How do I get 340?
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EierVonSatan
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(Original post by a.f.x.d)
How do I get 340?
mass/Mr x 2/3 (ratio in balanced equation) x Mr of ammonia
Last edited by EierVonSatan; 1 month ago
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scimus63
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https://www.science-revision.co.uk/m...equations.html

worked examples here
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