Final answer:
The theoretical yield of ammonium sulphate can be calculated from the amount of sulphuric acid using stoichiometric equations and the percent yield is determined by comparing the actual yield to the theoretical yield.
Step-by-step explanation:
In Chemistry, the theoretical yield is defined as the maximum amount of product that can be formed from the reactants in a chemical reaction, assuming perfect conditions and 100% efficiency in the reaction and product purification process. To calculate the theoretical yield of ammonium sulphate from a given amount of sulphuric acid (H₂SO₄), we use the stoichiometry of the balanced chemical equation and the molar mass of the substances involved.
For instance, if we start with 2.0 kg of sulphuric acid to produce ammonium sulphate, we first convert the mass of sulphuric acid to moles using its molar mass. Then, by using the mole ratio from the balanced equation, we calculate the moles of ammonium sulphate that can theoretically be produced. These moles are then converted to grams using the molar mass of ammonium sulphate:
- Calculate moles of H₂SO₄: mass (2.0 kg) divided by molar mass.
- Use stoichiometry to find moles of ((NH₄)₂SO₄).
- Calculate the expectant mass of ((NH₄)₂SO₄) using its molar mass.
The formula for percent yield is (actual yield)/(theoretical yield) × 100. If 2.2 kg of ammonium sulphate is the actual yield, we use the theoretical yield that we calculated to determine the percent yield. This helps in evaluating the efficiency and effectiveness of the reaction and purification process.