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

Question

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO3(s)?CaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 71.0L of carbon dioxide at STP? and Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is

2C4H10(g)+13O2(g)?8CO2(g)+10H2O(l)

At 1.00 atm and 23 ?C, what is the volume of carbon dioxide formed by the combustion of 2.00g of butane?

Explanation / Answer

CaCO3 --> CaO + CO2

100 gm of CaCO3 gives 22.4 L of CO2 at STP

So, to produce 71.0 L of CO2 requires 71.0 * (100/22.4) gm of CaCO3

which is 316.96 gm.

2C4H10 + 13O2 --> 8CO2 + 10H2O

implies 2 moles (2x58 gm) of Butane gives 8 moles of Carbon dioxide

So, 2 gm of Butane gives 8 * (2/116) moles of Carbon dioxide

Using the equation PV = nRT

where P = 1 atm, n = 8 * (2/116) moles, R = 0.08206 L atm mol

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

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