When heated, calcium carbonate decomposes to yield calcuim oxide and carbon diox

Question

When heated, calcium carbonate decomposes to yield calcuim oxide and carbon dioxide gas via the reaction CaCO_3(s) rightarrow CaO(s) + CO_2(g) What is mass of calcium carbonate needed to produce 25.0 L of carbon dioxide at STP? Express your answer with the appropriate units. Butane C_4H_10 is a component of natural gas that is used as a fuel for cigarette lighters. The balanced equation of the complete combusion of butane is 2C_4H_10(g) + 19O_2(g) rightarrow 8CO_2(g) + 10H_2O(l) At 1.00 atm and 23 degree C what is the volume of carbon dioxide formed by the combusion of 2.80 g of butane? Express your answer with the appropriate units.

Explanation / Answer

CaCO3 (s) -----> CaO (g) + CO2 (g)
number of moles of CO2 = PV /RT
                       = 1 *25/(0.0821*273)
                       = 1.1154 moles
1.1154 moles of CO2 requires 1.1154 moles of CaCO3
mass of CaCO3 = 1.1154 * 100 = 111.54 g

2 C4H10 + O2 -----> 8 CO2 + 10 H2O
2 moles of C4H10 produces 8 moles of CO2
2*58 g of C4H10 produces 8 *44 g of CO2
2.8 g of C4H10 produces (8*44)/(2*58)*2.8 g of CO2
                       = 8.496 g of CO2
Volume of CO2 = nRT/P = ((8.496/44)*0.0821*296)/1
Volume of CO2 = 4.6924 L

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.