Limestone (CaCO₃) emits CO₂ gas when exposed to HCl. What is the theoretical yield of CO₂ if 9.45 grams of limestone is completely dissolved in HCl?
CaCO₃( s ) + 2 HCl( aq ) → CaCl₂( aq ) + CO₂( g ) + H₂O( l )

Question

Quizplus · Accepted Answer

First, we need to correct the chemical formulas: CaCO3 (limestone) emits CO2 gas when exposed to HCl. The balanced chemical equation is: CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l). The molar mass of CaCO3 is approximately 100.09 g/mol, and the molar mass of CO2 is approximately 44.01 g/mol. Given 9.45 grams of CaCO3, we first find the moles of CaCO3: 9.45 g / 100.09 g/mol = 0.0944 mol. Since the reaction is 1:1 for CaCO3 to CO2, the moles of CO2 produced will also be 0.0944 mol. The mass of CO2 produced is then: 0.0944 mol * 44.01 g/mol = 4.15 g, which rounds to 4.16 g.

Limestone (CaCO3) Emits CO2 Gas When Exposed to HCl

Limestone (CaCO₃) Emits CO₂ Gas When Exposed to HCl