Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: n2 (g) + h2 (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



Free Class