Final answer:
The reaction between iron(III) sulfate and ammonia produces iron(III) hydroxide and ammonium sulfate. The percent yield is calculated using the mass of sulfuric acid and the actual yield of ammonium sulfate. Stoichiometry of the balanced chemical equation is used to determine theoretical yield.
Step-by-step explanation:
The reaction between iron(III) sulfate and ammonia is a multi-step process involving ion exchange and precipitation. Ammonia, when added to an aqueous solution of iron(III) sulfate, precipitates iron(III) hydroxide, following the formula:
Fe2(SO4)3 (aq) + 6NH4OH (aq) → 2Fe(OH)3 (s) + 3(NH4)2SO4 (aq)
The iron(III) hydroxide can then be filtered out, leaving ammonium sulfate in the solution. Moreover, calculating the theoretical yield of ammonium sulfate from sulfuric acid involves stoichiometry. Given that the sulphuric acid reacts with ammonia to produce ammonium sulfate, the theoretical yield can be calculated using the molar mass and coefficients from the balanced chemical equation:
H2SO4 + 2NH3 → (NH4)2SO4
To calculate the percent yield, we use the actual yield and theoretical yield obtained from the initial mass of sulphuric acid used:
Percent Yield = (Actual Yield / Theoretical Yield) x 100%
If 2.0 kg of H2SO4 is used, and the actual yield of fertilizer is 2.2 kg, we can determine the percent yield after calculating the theoretical yield based on the stoichiometry of the reaction.