This question is about the Haber process:
N2(g) + 3H2(g) ⇌ 2NH3(g)
The forward reaction is exothermic. 120 moles of hydrogen gas are mixed with 40.0 moles of nitrogen gas and pressurised. The mixture of gases is passed over an iron catalyst at 450 °C until the mixture reaches equilibrium. 20.0% of the reactants are converted to ammonia. The total volume of the mixture is 1.00 dm3.
a How many moles of nitrogen and of hydrogen remain at equilibrium? 
b How many moles of ammonia are formed? 
This can be done using
20/100 × 160 = 32 mol ammonia
80/100 × 120 = 96 mol hydrogen
80/100 × 40 = 32 mol nitogen
BUT PLEASE SOMEBODY SOLVE IT USING THE ICE TABLE METHOD. ILL BE GRATEFUL
Equilibria question please help
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- 17-05-2016 20:13
Last edited by Sriramkarthik; 17-05-2016 at 21:27. Reason: My previous answer was a mistake
- 17-05-2016 20:43
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- 17-05-2016 20:46
Is this GCSE/iGCSE or something that we could be asked in a GCSE exam or is it an AS question/A2 question?
- 17-05-2016 20:48
It is an AS chemistry question
- 18-05-2016 00:27
Please check my working of the ice table.
I dont know why am i getting wrong answer.
Please tell where am i wrong
The correct answer is ammonia 32
Which i dont seem to get through an ice table
- 18-05-2016 09:34
20% of the total reactants become products so 32 is the number of moles of NH3 and to form that many moles of NH3 the change in the number of moles of N2 and H2 is 20% too and 20% of each of their moles are 8 and 24 respectively. When you add them up you get the moles of NH3 formed therefore conserving the number of moles in the eqn.
Hope that helps.
- 18-05-2016 09:40
Yes i got that but please tell what will be the value of X in our ice table?
I seem to get that wrong that is why my answer is wrongLast edited by Insia786; 18-05-2016 at 09:41.
- 18-05-2016 09:47