Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from N₂ and H₂ by the Haber

Question

Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from
N₂ and
H₂ by the Haber process. Because the reaction reaches equilibrium before going completely to product, the stoichiometric amount
of ammonia is not obtained. At a particular temperature and pressure,
10.0 g of
H₂ reacts with
20.0 g of
N₂ to form ammonia. When equilibrium is reached,
15.0 g of
NH3 has formed. (a) Calculate the percent yield. (b) How many moles of
N₂ and
H₂ are present at equilibrium?

Kunduz · Accepted Answer

Click to see the answer