Dinitrogen and dihydrogen react with each other to produce ammonia according to following chemical equation: N2 (g) + 3H2 (g) →2NH3 (g) (a) Calculate the mass of ammonia gas formed if 2.0 kg of nitrogen gas reacts with 1.0 kg of hydrogen gas. (b) Which of the two reactants is the limiting reagent and why? (c) Which of the two reactants will remain un-reacted and what will be the amount left un-reacted?
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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
=571.43g
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