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Butane is used as a fuel in gas grills, and produces heat by the following reaction. 2C4H10(g) + 13O2(g) ĺ 8CO2(g) + 10H2O(l), ǻH°rxn= –5,314 kJ/mol. How many liters of CO2 are produced per 1.00 × 10^4 kJ of heat released? Assume STP and show all work

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13 Dec 2019
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Related questions

The combustion of butane produces heat according to theequation
2C4H10(g) + 13O2 (g) ==> 8CO2(g) +10H2O(l) [Delta H°rxn=-5,314kJ/mol]
How many grams of CO2 are produced per 10000 kJ of heat released?

1- When heated, calcium carbonate decomposes to yield calcium oxideand carbon dioxide gas via the reaction

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

Whatis the mass of calcium carbonate needed to produce51.0Lof carbon dioxide at STP?






2- Butane,

C4H10,is a component of natural gas that is used as fuel for cigarettelighters. The balanced equation of the complete combustion ofbutane is

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

At 1.00 atmand 23 ?C,what is the volume of carbon dioxide formed by the combustion of1.00gof butane?


The ideal gas law : PV=nRT relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 L⋠atm/(K⋠mol)or 8.3145 J/(K⋠mol). The equation can be rearranged as follows to solve for n: n=PVRT

1. 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 75.0 L of carbon dioxide at STP?

2. 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 3.80 g of butane?

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