10th Class Chemistry Chapter 3 Test03. Stoichiometry

Q1. Multiple choice questions (Attempt all · 10 × 1 = 10)

1. One mole of $H_2O$ has a mass of:
   1. 10 g
   2. 18 g
   3. 16 g
   4. 23 g
2. A solution has a strength of 50 g/dm³. Expressed in g/cm³ it is:
   1. 0.05 g/cm³
   2. 0.5 g/cm³
   3. 5 g/cm³
   4. 0.005 g/cm³
3. The yield actually obtained from a reaction is called:
   1. Theoretical yield
   2. Practical yield
   3. Actual yield
   4. Experimental yield
4. The empirical formula of a compound represents:
   1. Actual ratio of atoms
   2. Simplest whole-number ratio of atoms
   3. Mass ratio of elements
   4. The molecular structure
5. What does “18M H₂SO₄” mean?
   1. 18 g of H₂SO₄ in 1 dm³ solution
   2. 18 moles of H₂SO₄ in 1 dm³ solution
   3. 18% solution of H₂SO₄
   4. 18 cm³ of H₂SO₄ in solution
6. Formula of dilution is:
   1. M₁V₁ = M₂V₂
   2. M = mass / moles
   3. S = mass of solute / volume of solution
   4. P = (actual mass / total mass) × 100
7. In titration, the end point is detected when:
   1. Color of solution becomes darker
   2. Indicator shows color change
   3. Solution evaporates
   4. The solution is heated
8. The yield calculated from a balanced chemical equation is called:
   1. Actual yield
   2. Theoretical yield
   3. Percent yield
   4. Practical yield
9. Which is the SI unit of the amount of substance?
   1. Gram
   2. Mole
   3. Kilogram
   4. Atom
10. If 25 g NaOH is dissolved to make 1 dm³ of solution, molarity is:
    1. 0.5 M
    2. 1.0 M
    3. 2.0 M
    4. 0.25 M