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
THESE ARE CORRECT ANSWERS
SOMEONE DO THIS USING THE ICE TABLE PLEASE.
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- Thread Starter
- 18-05-2016 02:17
- 18-05-2016 08:09
Or at least show us what you've tried.