Balanced the equation.
2C4H10 + 14O2 ==> 8CO2 + 10H2O
Convert 125 g oxygen to butane.
450 g oxygen/32 = moles oxygen = about 14 moles but you need to be more accurate.
Now use the coefficients in the balanced equation and convert moles O2 to moles C4H10 this way.
14 moles O2 x (2 moles C4H10/14 moles O2) = 14 x (2/14) = about 2 moles C4H10. Convert that to grams C4H10
moles x molar mass = grams. I get approximately 116 g C4H10 which means you can burn about 116 g butane so that is almost but not quite enough oxygen.
Is 450g of oxygen enough to burn 125g of butane according to the following equation? C4H10 + O2 ---> CO2 + H2O? show why or why not?
2 answers
3=1