Class 10 Chemistry Chapter 15 Stoichiometry Test 4 – 2027 | Solved Paper
Grade 10 Chemistry chapter 15 Test 4 with answers
Prepare for the Punjab Board Class 10 Chemistry examination with the Chapter 15: Stoichiometry Class Test 4 from the Punjab Board 2027 Model Papers. This test is designed to help students revise important Stoichiometry concepts, chemical equations, numerical problems, and related Chemistry questions. Practice this Class 10 Chemistry Chapter 15 Test 4 to strengthen your conceptual understanding and improve your preparation for the Punjab Board annual examination 2027.
CHAPTER WISE CLASS TEST
(Test # 4)
Find out the concentration of H2SO4 in mol/dm3 if its 10 cm3 react with 20 cm3 of NaOH solution having concentration 0.1 mol/dm3.
The empirical formula of magnesium chloride is:
If the molar mass of a compound is 178 g/mol and its empirical formula is C3H5O3. What is its molecular formula?
The reactant which is consumed completely in a chemical reaction is called:
When natural gas burns in air, which component is the limiting reactant?
The theoretical yield of Zn(NO3)2 from 0.76 mol of Zn is:
If the actual yield of a compound is 0.198 g while the theoretical yield is 0.217 g. What will be the percentage yield?
The formula to calculate percentage yield is:
(PART – I)
- Why is percentage yield important?
It shows the efficiency of a reaction by comparing actual yield with theoretical yield, helping chemists and industries judge cost, waste and the best conditions for a process.
- How can molecular formula of a compound be calculated?
Find the empirical formula mass, divide the given molar mass by it to get n, then multiply every subscript of the empirical formula by n: Molecular formula = (Empirical formula)n.
- Will there be a limiting reactant in a reversible reaction?
No. In a reversible reaction the reaction does not go to completion, so no reactant is consumed completely and a true limiting reactant does not arise.
- How does the limiting reactant control the amount of product formed?
The reaction stops when the limiting reactant is used up, so the amount of product is fixed by the moles of the limiting reactant according to the balanced equation.
- How do you know if a formula is empirical or not?
If the subscripts of all atoms have no common factor (simplest whole-number ratio), it is empirical. If they can all be divided by a common number, it is not (e.g. C6H12O6 → CH2O).
- What is percentage yield and write its formula?
Percentage yield is the ratio of actual yield to theoretical yield expressed as a percentage.
% Yield = (Actual yield ÷ Theoretical yield) × 100
(PART – II)
- the mole ratio of reactants and products (e.g. 2H2 + O2 → 2H2O);
- the masses of reactants needed or products formed, using molar masses;
- volumes of gases at STP (1 mol = 22.4 dm3);
- the limiting reactant, and hence theoretical and percentage yield;
- the number of particles involved (1 mol = 6.02 × 1023).
