Butane, , is a component of natural gas that is used as fuel for cigarette lighters.At 1.00 and 23 , how many liters of carbon dioxide are formed by the combustion of 1.00 of butane?

Do you mean 1.0 atm and 23 C ? What about the 1.00 of butane? What is that?

Numbers without units are no help.

Butane is C2H6. Write the balanced equation of combustion. Then compute the moles of CO2 formed. Then convert that to liters.

To determine the number of liters of carbon dioxide formed by the combustion of 1.00 gram of butane (C4H10), we need to use the balanced chemical equation for the combustion of butane.

The balanced equation for the combustion of butane is as follows:

C4H10 + 13/2 O2 -> 4 CO2 + 5 H2O

From the equation, we can see that for every 1 mole of butane (C4H10) reacted, we produce 4 moles of carbon dioxide (CO2). The molar mass of butane (C4H10) is approximately 58.12 grams/mol.

To calculate the number of moles of butane in 1.00 gram:

Number of moles = Mass / Molar mass

Number of moles of butane = 1.00 g / 58.12 g/mol

Now, we can calculate the number of moles of carbon dioxide produced using the stoichiometry of the balanced equation:

Number of moles of carbon dioxide = Number of moles of butane × (4 moles CO2 / 1 mole butane)

Finally, to convert the number of moles of carbon dioxide to liters, we need to use the ideal gas law, assuming the ideal gas behavior:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L.atm/mol.K), and T is the temperature in Kelvin (23 °C = 23 + 273 = 296 K).

To calculate the volume in liters:

Volume (V) = Number of moles × R × T / P

Substitute the values into the equation to find the volume of CO2 in liters. Assuming the pressure (P) is 1.00 atm:

Volume (V) = Number of moles × 0.0821 L.atm/mol.K × 296 K / 1.00 atm