Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: N2(g) + 3H2(g) →2NH3(g) (i) calculate the mass of ammonia produced if 2.00 × 10^3 g dinitrogen reacts with 1.00 × 10^3 g of dihydrogen. (ii) will any of the two reactants remain unreacted? if yes which one ?(iii) what would be its mass?

N2(g) + 3H2(g) →2NH3(g)

28g        6g               34g


28 g of N2 reacts with 6g of H2.


1g of N2 reacts with 6/28 g of H2


2000g of N2 will react with 2000 × 6/28


= 428.57 of H2


but H2 is given 1 × 10³g is greater than 428.57 g


N2 is a limiting reagent and limits the production of ammonia


28g of N2 produces 34 g of NH3


1g of N2 produces 34/28 g of NH3


2000g of N2 will produce 34/28 × 2000


= 2428.57 g of NH3.


(ii) H2 is excess so it remains unreacted


(iii) Mass of unreacted dihydrogen = 1000-428.57



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