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Class 11  »  Chemistry  »  Some Basic Concepts of Chemistry

Limiting Reagent - UNSOLVED PRACTICE SET

Class 11

Chapter: Some Basic Concepts of Chemistry | Topic: Limiting Reagent

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Class 11

LIMITING REAGENT - UNSOLVED PRACTICE SET

Topic: Limiting Reagent

Time: 40 mins | Marks: 30 | Difficulty: Medium

Multiple Choice Questions

Q1. The limiting reagent in a chemical reaction is:

  1. The reactant present in the largest amount
  2. The reactant that is completely consumed first and limits the amount of product
  3. The reactant that remains unreacted
  4. The product formed in the smallest amount

Q2. In the reaction H₂ + Cl₂ → 2HCl, if 2 g H₂ is mixed with 71 g Cl₂, the limiting reagent is:

  1. H₂
  2. Cl₂
  3. Both are in exact stoichiometric ratio
  4. Cannot be determined

Q3. If 10 g of hydrogen and 64 g of oxygen are mixed to form water, the amount of water formed is limited by:

  1. Hydrogen
  2. Oxygen
  3. Both equally
  4. Neither

Q4. The excess reagent is:

  1. The reactant that gets completely used up
  2. The reactant that remains after the reaction stops
  3. The product that forms in excess
  4. The catalyst used in excess

Q5. In a reaction between 1 mole of A and 2 moles of B to form 1 mole of C, if 0.5 mole of A is mixed with 1.5 moles of B:

  1. A is the limiting reagent
  2. B is the limiting reagent
  3. Neither is limiting
  4. Both are limiting

Q6. The amount of product formed in a reaction is always determined by:

  1. The excess reagent
  2. The limiting reagent
  3. The total mass of all reactants
  4. The volume of the container

Short Answer Questions

Q7. Define limiting reagent. Why is it important to identify the limiting reagent in industrial chemical processes?

Q8. In the reaction 2H₂ + O₂ → 2H₂O, 4 g of H₂ reacts with 40 g of O₂. Identify the limiting reagent.

Q9. What is an excess reagent? How does it differ from the limiting reagent?

Q10. Why does the amount of product formed depend on the limiting reagent and not on the excess reagent?

Q11. Your mother wants to make 20 chapatis. She has 500 g of flour (enough for 25 chapatis) but only 200 mL of water (enough for 15 chapatis). How many chapatis can she actually make? Which ingredient is the "limiting reagent" in this kitchen chemistry?

Q12. In the reaction N₂ + 3H₂ → 2NH₃, if 28 g of N₂ and 10 g of H₂ are taken, which is the limiting reagent? Calculate the mass of NH₃ formed.

Long Answer Questions

Q13. Explain the concept of limiting reagent with a suitable example. Describe the steps to identify the limiting reagent in a chemical reaction. In the reaction:

2Al + 3Cl₂ → 2AlCl₃

5.4 g of aluminium is reacted with 21.3 g of chlorine. Identify the limiting reagent and calculate the mass of aluminium chloride formed.

(Atomic masses: Al = 27 u, Cl = 35.5 u)

Q14. Define limiting reagent and excess reagent. For the reaction:

CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂

10 g of CaCO₃ is reacted with 10 g of HCl.

(a) Calculate the number of moles of each reactant.

(b) Identify the limiting reagent.

(c) Calculate the mass of CaCl₂ formed.

(d) Calculate the mass of the excess reagent left unreacted.

(Atomic masses: Ca = 40 u, C = 12 u, O = 16 u, H = 1 u, Cl = 35.5 u)

Q15. A chemistry teacher demonstrates the reaction between zinc and sulphuric acid in class:

Zn + H₂SO₄ → ZnSO₄ + H₂

She takes 13 g of zinc granules and adds 200 mL of 0.5 M H₂SO₄ solution.

(a) Calculate the number of moles of zinc and sulphuric acid.

(b) Identify the limiting reagent.

(c) Calculate the volume of hydrogen gas produced at STP.

(d) If the teacher wants to ensure that zinc is completely consumed, what minimum molarity of H₂SO₄ should she use for 200 mL solution?

(Atomic masses: Zn = 65 u, S = 32 u, O = 16 u, H = 1 u)

Numerical / Application-Based Problems

Q16. For the combustion of propane: C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

44 g of propane is burned in a cylinder containing 160 g of oxygen.

(a) Identify the limiting reagent.

(b) Calculate the mass of CO₂ produced.

(c) Calculate the mass of the excess reagent remaining.

(Atomic masses: C = 12 u, H = 1 u, O = 16 u)

Q17. In the reaction: 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

A student mixes 200 mL of 2 M NaOH with 150 mL of 1 M H₂SO₄.

(a) Calculate the number of moles of NaOH and H₂SO₄.

(b) Identify the limiting reagent.

(c) Calculate the mass of Na₂SO₄ formed.

(d) Calculate the molarity of the excess reagent remaining in the solution.

(Atomic masses: Na = 23 u, S = 32 u, O = 16 u, H = 1 u)

Q18. A factory produces ammonia using the Haber process: N₂ + 3H₂ → 2NH₃

Daily supply: 1000 kg of N₂ and 200 kg of H₂.

(a) Identify the limiting reagent.

(b) Calculate the theoretical mass of NH₃ produced per day.

(c) If the factory achieves 90% yield, calculate the actual mass of ammonia produced.

(d) How much additional H₂ must be supplied to completely utilize the N₂?

(Atomic masses: N = 14 u, H = 1 u)


Total: 30 Marks | Time: 40 mins

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Importance and Scope of Chemistry Laws of Chemical Combination Daltons Atomic Theory Atomic and Molecular Mass Mole Concept and Molar Mass Percentage Composition and Empirical Formula Stoichiometry and Stoichiometric Calculations Concentration Terms Molarity Molality Normality Mole Fraction