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Butane,C4H10 , is a component of natural gas that is used as fuel for cigarette lighters.At 1.00atm and 23 degrees Celsius , how many liters of carbon dioxide are formed by the combustion of 1.00 of butane?

2C4H10+13O2 yields 8CO2+10H2o

Any help would be greatly appreciated

2 answers

You have the balanced equation. Is the butane at the same P and T as CO2? Is that 1.00 liters of butane or some other unit?
Use PV = nRT. You have pressure, you have volume of butane (must be in liters), you know R, and T is 23 degrees C but don't forget to change to Kelvin. Calculate n, the number of mols of butane you start with.
Second part. Use the coefficients in the balanced equation to change mols butane to mols CO2, then use PV = nRT to calculate volume CO2. Post your work if you get stuck.
13.26