hmm.. would it be one? (because there's one mole of carbon and one of oxygen?) I'm not too sure
Nope
You have the right sort of idea though. The equation shows that for every one mole of carbon burned, one mole of CO2 would form - the mole ratio is 1:1. As you have 0.05 moles of carbon, the number of moles of carbon dioxide would also be the same (0.05).
So you have the number of moles of CO2, you can work out it's Mr quickly and you can use Mass = Mr x Moles to work out the mass.
Since you have 0.05mol of CO2 (as mentioned previously), to work out the Mass of CO2 produced, you must use the following equation: mass=number of moles*Relative Molecular mass. The Mr of CO2 is 12(Carbon)+(2*16(Oxygen))=44 Seeing as you now have the Mr(44) of CO2 all you have to do is multiply that by 0.05mol as the ratio 1:1. Which gives you the total mass of CO2 produced 2.2g I hope I didnt confuse you more because I got stuck on this for a little bit too but I read back pages 33-38 in AS Chemistry AQA text book and everything came back