Ask Question
22 May, 00:51

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)

+2
Answers (1)
  1. 22 May, 03:27
    0
    Yield of CO₂ = 79.1 %

    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%
Know the Answer?
Not Sure About the Answer?
Get an answer to your 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 ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers