Question

When 10.9 g CaCO3 reacts with excess hydrochloric acid, as below, 3.79 g of CO2 is produced. What is the percent yield of CO2? Do not type the units with your answer. CaCO3(s) + HCl(aq) => CO2(g) + CaCl2(aq) + H2O(l) (not balanced)

Answer 1

Yield of CO₂ = 79.1 %

Step-by-step explanation:

This is the balanced reaction:

CaCO₃ (s) + 2HCl (aq) → CO₂ (g) + CaCl₂ (aq) + H₂O (l)

As the hydrochloric acid is in excess, the limiting reactant is the CaCO₃.

Let's convert the mass to moles

10.9 g / 100.08 g/mol = 0.109 moles

Ratio is 1:1, so 0.109 moles of CaCO₃ will produce the same amount of CO₂.

Let's determine the mass

0.109 moles of CO₂ . 44 g/mol = 4.79 g

Now, we can determine the yield

(yeild produced / theoretical yield) . 100 =

(3.79 / 4.79) . 100 = 79.1%