Butane, C_{4}H_{10}, 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 C_{4}H_{10}(g) + 13 O_{2}(g) → 8 CO_{2}(g) + 10 H_{2}O(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*:

$\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}$

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

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