Ammonia is produced by the millions of tons annually for use as 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, 12.17 g h2 reacts with 24.34 g n2 to form ammonia. when equilibrium is reached, 23.24 g nh3 has formed.
(a) calculate the percent yield,
(b) how many moles of n2 and h2 are present at equilibrium?
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