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Question

a)  Calculate the mass of ammonia produced if 2.00 ×10g of nitrogen reacts with 1.00 ×10g. 

b) Will any of the two reagents will remain unreacted. If yes, which one and what would be its mass. 


Solution

N2(g) + H2(g) → 2NH3(g)

Balancing the chemical equation, From the equation, 1 mole (28 g) of N2 reacts with 3 mole (6 g) of H2 to give 2 mole (34 g) of ammonia. ⇒ 2.00 × 10^3g of N2 will react with H2 i.e.,2.00 × 10^3g of N2 will react with 428.6 g of H2 Given, Amount of H2= 1.00 × 103g Hence, N2 is the limiting reagent. 28 g of N2 produces 34 g of NH3. Hence, mass of ammonia produced by 2000 g of N2= 2428.57 g N2 is the limiting reagent and H2 is the excess reagent. Hence, H2 willremain unreacted. Mass of H2 left unreacted = 1.00 × 103g – 428.6 g= 571.4 g

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