Practice Theoretical Yield in Chemistry
Use these practice problems to test your method after reviewing the concept explanation and worked examples.
Quick Recap
The maximum amount of product that could form based on stoichiometry and the limiting reactant.
The perfect-world result — the most product you could possibly get if nothing is lost or wasted.
Example 1
easyDefine theoretical yield and explain how it differs from actual yield.
Example 2
mediumCalculate the theoretical yield of water when 8.0 g of hydrogen reacts with excess oxygen. (2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}; H = 1.008, O = 16.00\,\text{g/mol})
Example 3
mediumIn the reaction 2\text{Na} + \text{Cl}_2 \rightarrow 2\text{NaCl}, calculate the theoretical yield of NaCl from 11.5 g of sodium with excess chlorine. (Na = 23.0, Cl = 35.45\,\text{g/mol})
Example 4
hardA student reacts 6.50 g of zinc with 20.0 mL of 3.00\,\text{M HCl}. The reaction is \text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2. Determine the limiting reactant and the theoretical yield of \text{ZnCl}_2. (Zn = 65.38, \text{ZnCl}_2 = 136.28\,\text{g/mol})