Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical reaction: N 2 g + 3 H 2 g → 2 NH 3 g (i) Calculate the mass of ammonia produced if 2.00 × 1 0 3 g dinitrogen reacts with 1.00 × 1 0 3 g of dihydrogen. (ii) Will any of the two reactants remain unreacted? (iii) If yes, which one and what would be its mass?

Given: Mass of dinitrogen = 2.00 × 1 0 3 g Balancing the given chemical equation, N 2 g + 3 H 2 g → 2 NH 3 g (i) From the equation, 1 mole 28 g of nitrogen reacts with 3 moles 6 g of dihydrogen to give 2 moles 34 g of ammonia. 2 . 00 × 10 3 g of N 2 react with 6 2 × 10 3 28 g of H 2 i.e., 428 . 6 g of H 2 . Given amount of H 2 is 1 . 00 × 10 3 g . 28 g of N 2 produces 34 g of NH 3 Therefore, the mass of Ammonia produced by 2000 g of N 2 is 34 g 28 g × 2000 g = 2428 . 6 g . (ii) H 2 is the excess reagent. Therefore, H 2 will not react. (iii) Mass of dihydrogen unreacted = Given mass of dihydrogen - Reacted mass of dihydrogen = 1 × 10 3 - 428 . 6 = 571 . 4 g

E M B I B E

Textbook for Class XI Chemistry Part I>Chapter 1 - Some Basic Concepts of Chemistry>EXERCISES>Q 1.23

EASY

11th CBSE

IMPORTANT

Earn 100

In a reaction $A + B_{2} \to {AB}_{2}$
Identify the limiting reagent, if any, in the following reaction mixture.
$2.5$ moles $A + 5$ mole $B$ .

Important Questions on Some Basic Concepts of Chemistry

HARD

11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 1 - Some Basic Concepts of Chemistry>EXERCISES>Q 1.24

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical reaction:
$N_{2} (g) + 3 H_{2} (g) \to 2 {NH}_{3} (g)$
(i) Calculate the mass of ammonia produced if $2.00 \times 1 0^{3} g$ dinitrogen reacts with $1.00 \times 1 0^{3} g$ of dihydrogen.