What volume in liters of oxygen is needed to burn all the butane at 0.850 atm and 25 degrees Celsius?

Question

Can you please show me step by step on how to get this answer?

The tank contains 55.2 g butane
Butane is used to fill gas tanks for heating. The following equation describes its combustion

2CH410(g) + 13O2(g) -- 8CO2(g) + 10H2O(g)

Answer 1

First you need to do the stoichiometry.

Convert the 55.2 g of butane to moles by dividing the mass by the molecular mass.

Th emolare ratio is 13 O2 / 2 butane, so multiply th emoles of butane by 13/2 to get moles of oxygen.

Now use the conversion of 1 mole = 22.4 liters of gas at STP.

Take the number of moles of oxygen and multiply by 22.4 liters.

The last step is to use the gas laws to convert the liters of O2 from STP to your actual conditions. Don't forget to use Kelvin for the T and not celsius. Convert from 1 atm. to 0,850 atm and from 273 K to 298K.