hi i urgently need help. I am having trouble with this question please explain thoroughly.
Ammonia is produced from nitrogen and hydrogen. the equation for this reaction is
N29(g) + 3H2(g) = 2NH3(g)
(i) a company wants to make 6.8 tonnes of ammonia
calculate the mass of nitrogen needed
relative atomic masses (Ar) H=1 , n=14
(ii) the company expected to make 6.8 tonnes of ammonia.
the yield of ammonia was only 4.2 tonnes
calculate the percentage yield of ammonia
(iii) use the equation above to explain why the percentage yield of ammonia was less than expected.
chemistry help needed Watch
- Thread Starter
- 29-01-2017 15:58
- 29-01-2017 15:59
What have you done so far?
- 29-01-2017 16:01
What is the molecular mass of ammonia?
How many moles of ammonia do you have in 6.8 tonnes?
How many moles of nitrogen do you need for each mole of ammonia?
If you answer the above questions then you have basically answered question 1i