Question 24 of 36intermediate🔧 ApplyNumerical5 marks

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 2.00×102.00 \times 10³ g dinitrogen reacts with 1.00×101.00 \times 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)
Answer

The mass of ammonia produced is 2.43×1032.43 \times 10^3 g.

(ii)
Answer

Yes, one of the two reactants will remain unreacted.

(iii)
Answer

Dihydrogen (H2\text{H}_2) remains unreacted, and its mass would be 0.568×1030.568 \times 10^3 g.

Explanation

To solve this, we first write the balanced chemical equation: N2(g)+3H2(g)→2NH3(g)\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightarrow 2\text{NH}_3(\text{g}). We calculate the moles of dinitrogen and dihydrogen given. By comparing the mole ratio required by the balanced equation with the available moles, we identify the limiting reagent. The amount of product formed is determined solely by the limiting reagent. The excess reactant is the one that remains unreacted, and its remaining mass is calculated by subtracting the consumed amount from the initial amount.

PreviousNext