Calcium Carbonate Lab Experiment Concepts

In this lab tutorial, students learn to produce calcium carbonate (chalk) by reacting sodium carbonate monohydrate with calcium chloride. The process involves calculating the required grams of reactants, converting these to moles, and using stoichiometry to determine the necessary quantities. The video demonstrates mixing the reactants, observing the formation of chalk, and filtering the product. Finally, the tutorial covers calculating the percent yield of the reaction, emphasizing the importance of accurate measurements and calculations.

What is the primary goal of the lab experiment?

• To produce sodium chloride

• To create calcium carbonate

• To generate carbon dioxide

• To synthesize sodium carbonate

What is the target amount of calcium carbonate to be produced in the lab?

• 1.0 grams

• 2.0 grams

• 3.0 grams

• 4.0 grams

How do you calculate the number of moles of calcium carbonate needed?

• By dividing the grams of calcium carbonate by 100

• By multiplying the grams of calcium carbonate by 100

• By subtracting the grams of calcium carbonate from 100

• By adding the grams of calcium carbonate to 100

What is the molar mass of sodium carbonate monohydrate used in the calculations?

• 124 g/mol

• 200 g/mol

• 150 g/mol

• 100 g/mol

What is the purpose of using a filter paper in the experiment?

• To dissolve the reactants

• To collect the calcium carbonate

• To measure the temperature

• To increase the reaction rate

Why is it important to rinse the calcium carbonate with distilled water?

• To remove excess reactants

• To prevent salt contamination

• To speed up drying

• To increase the yield

What was the actual yield of calcium carbonate obtained in the experiment?

• 2.00 grams

• 3.00 grams

• 1.57 grams

• 2.40 grams

How is the percent yield of the reaction calculated?

• By dividing the actual yield by the theoretical yield and multiplying by 100

• By multiplying the actual yield by the theoretical yield

• By subtracting the actual yield from the theoretical yield

• By adding the actual yield to the theoretical yield

What was the percent yield of calcium carbonate in the experiment?

• 78.5%

• 100.0%

• 50.0%

• 90.0%

What could cause an artificially high yield in the experiment?

• Loss of product during filtration

• Presence of impurities

• Excess water in the product

• Incomplete reaction