1.24 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 × 103 g dinitrogen reacts with 1.00 ×103 g of dihydrogen.
(ii) Will any of the two reactants remain unreacted?
(iii) If yes, which one and what would be its mass?
(i) Balancing the given chemical equation,
From the equation, 1 mole (28 g) of dinitrogen reacts with 3 moles (6 g) of dihydrogen to give 2 moles (34 g) of ammonia.
⇒ 2.00 × 103 g of dinitrogen will react with dihydrogen i.e., 2.00 × 103 g of dinitrogen will react with 428.6 g of dihydrogen.
Given, the Amount of dihydrogen = 1.00 × g Hence,
N2 is the limiting reagent.
28 g of N2 produces 34 g of .
Hence, the mass of ammonia produced by 2000 g of N2 = 2428.57 g
(ii) N2 is the limiting reagent and H2 is the excess reagent. Hence, H2 will remain unreacted.
(iii) Mass of dihydrogen left unreacted = 1.00 × g – 428.6 g = 571.4 g
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