Problem: 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 is2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(l)At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 2.00 g of butane?Express your answer with the appropriate units.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=PVRTThis equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

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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

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

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

Express your answer with the appropriate units.


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

This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.