Identify the apparatus and chemicals used in the experiment. Write the balanced chemical equation for the decomposition of calcium carbonate. Explain the observations and conclusions drawn from the re

i.
I: Alcohol burner
II: Retort stand
III: Test tube
IV: Delivery tube
V: Conical flask

ii.

• $\text{CaCO}_3$: Calcium carbonate
• $\text{CuSO}_4$: Copper(II) sulfate
• $\text{Ca(OH)}_2$: Calcium hydroxide

iii.
a. When wet calcium carbonate is strongly heated, the water will evaporate first. Then, the calcium carbonate will decompose into calcium oxide and carbon dioxide gas.
b. The balanced chemical equation is:

$$\text{CaCO}_3(\text{s}) \xrightarrow{\text{heat}} \text{CaO}(\text{s}) + \text{CO}_2(\text{g})$$

iv.
a. The anhydrous $\text{CuSO}_4$ (white) will turn blue in the presence of water vapor, indicating that water was produced from the wet $\text{CaCO}_3$.
b. The $\text{Ca(OH)}_2$ solution (limewater) will turn milky/cloudy due to the formation of insoluble calcium carbonate precipitate, indicating the presence of carbon dioxide gas.

v.
Anhydrous cobalt(II) chloride paper (changes from blue to pink in the presence of water).