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Question

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 2.00×103g dinitrogen reacts with 1.00×103g of dihydrogen.
(ii) Will any of two reactants remain unreacted?
(iii) If yes, which one and what would be its mass?

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Solution

(i) 1 mole of N2 produces 2 mole NH3
2×1032 mole produce =1037 mole NH3
3 mole of H2 produce 2 mole NH3
1032 mole produce =3×10322×1033×2 mole NH3
Clearly N2 is limiting regent and hence amount of NH3
produced =10007=140.86g
(ii) H2 will remain unreacted.
(iii) 1 mole of N2 react with 3 mole of H2
2×10328 mole of N2 will react with =3×2×1028=214.29g
Amount unreacted =1000214.29
=785.71g


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