Answer:
A. CaCO₃(s) → CaO(s) + CO₂(g).
B. Decomposition reaction.
C. 29.46 g.
D. 93.94%
Step-by-step explanation:
A. Write the balanced the reaction
- Calcium carbonate breaks down according to the balanced equation:
CaCO₃(s) → CaO(s) + CO₂(g),
1.0 mol of CaCO₃ is decomposed to produce 1.0 mol of CaO and 1.0 mol of CO₂.
B. Identify the reaction type (single replacement, double replacement, synthesis, decomposition or combustion).
- It is a decomposition reaction.
A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more elements or new compounds.
Herein, CaCO₃ is decomposed to produce CaO and CO₂.
C. What is the theoretical yield of carbon dioxide gas (in grams)?
- Firstly, we should get the no. of moles (n) of 67.00 grams of calcium carbonate:
n = mass/molar mass = (67.0 g)/(100.08 g/mol) = 0.6695 mol.
Using cross-multiplication:
1.0 mol of CaCO₃ produces → 1.0 mol of CO₂, from stichiometry.
∴ 0.6695 mol of CaCO₃ produces → 0.6695 mol of CO₂.
- We can calculate the theoretical yield of carbon dioxide gas using the relation:
∴ The theoretical yield of carbon dioxide gas = n*molar mass = (0.6695 mol)(44.0 g/mol) = 29.46 g.
D. What is the percent yield if 27.67 grams of carbon dioxide gas are actually produced?
∵ the percent yield = (actual yield/theoretical yield)*100.
actual yield = 27.67 g, theoretical yield = 29.46 g.
∴ the percent yield = (27.67 g/29.46 g)*100 = 93.94%.