In lab next week Ca(OH)_2 will be used to absorb your exhaled CO_2 to form CaCO_

Question

In lab next week Ca(OH)_2 will be used to absorb your exhaled CO_2 to form CaCO_3. If 50.0 g of Ca(OH)_2 and 50.0 g of CO_2 react what is the limiting reactant, excess reactant, and theoretical yield of CaCO_2? Ca(OH)_2(aq) + CO_2(g) rightarrow CaCO_3(s)+H_2O(l) a. What is the percent yield if 60.5 g of CaCO_3 was produced in the experiment? Write the molecular equation for the reaction that occurs during the production of chalk when an aqueous solution of calcium chloride and an aqueous solution of sodium carbonate react. For the following reaction write its complete ionic equation. AI_2(SO_4)_3 (aq) + 3 BaCl_2 (aq) rightarrow 2 AlCl_3 (aq) + 3 BaSO_4 (s) For the reaction in problem 3 write the net ionic equation

Explanation / Answer

Question 1

Balanced equation:
Ca(OH)2 + CO2 ===> CaCO3 + H2O
Reaction type: double replacement

50 gm of Ca(OH)2   = 50 / 74.09 = 0.6748 Moles

50 gm of CO2 = 50 / 44 = 1.13611 Moles

Limiting reagent is Ca(OH)2 because it is present as less moles.

Excess reaegnt is CO2 = 50-29.69 = 20.31 gm CO2 will be excess

Moles of CaCO3 to be produced = 0.6748 Moles

Mass of CaCO3 to be produced = 0.6748 Moles x 100.08 g/ moles = 67.54 gm

Theoretical yield = 67.54 gm

Percentage yield = 60.5 x 100 / 67.54 = 89.57 %

Question 2

Reaction between CaCl2 and Na2CO3 to produce Chalk and sodium chloride

Balanced equation:
CaCl2 + Na2CO3 ===> CaCO3 + 2 NaCl
Reaction type: double replacement

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