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?
2C4H10+13O2 yields 8CO2+10H2o
At 1.00 and 23 what?
1.00 what of butane?
To find the number of liters of carbon dioxide formed by the combustion of 1.00 mole of butane (C4H10), we need to use the stoichiometry of the balanced chemical equation provided.
The balanced equation is: 2C4H10 + 13O2 → 8CO2 + 10H2O
From the equation, we can see that for every 2 moles of butane, 8 moles of carbon dioxide are produced.
Given that we have 1.00 mole of butane, we can set up a proportion to find the number of moles of carbon dioxide produced:
2 moles of butane / 8 moles of carbon dioxide = 1.00 mole of butane / x moles of carbon dioxide
Simplifying the proportion:
2/8 = 1.00/x
2x = 8
x = 8/2
x = 4
So, 4 moles of carbon dioxide are formed by the combustion of 1.00 mole of butane.
Now, to convert moles of carbon dioxide to liters, we can use the ideal gas law: PV = nRT
Given:
Pressure (P): 1.00 atm
Temperature (T): 23 degrees Celsius = 23 + 273 = 296 K (converted to Kelvin using the formula K = °C + 273)
Number of moles (n): 4 moles
R is the ideal gas constant (0.08206 L·atm/(mol·K)).
Using the ideal gas law:
PV = nRT
V = (nRT) / P
V = (4 mol * 0.08206 L·atm/(mol·K) * 296 K) / 1.00 atm
V = 9.63 Liters
Therefore, when 1.00 mole of butane is combusted at 1.00 atm and 23°C, it will produce 9.63 liters of carbon dioxide.