Iron is produced from its ore by the reactions:2C(s) + O2(g) --gt; 2CO(g)Fe2O3(s) + 3CO(g) --gt; 2Fe (s) + 3CO2(g)How many moles of O2(g) are needed to produce 1 mole of Fe(s)?How would you go about figuring this out?
The easiest way is to get both the equations to have commom molar quantities. You want to go from Oxygen to iron via CO In the second equation, 2mol Fe are produced from 3mol CO But in the first equation, you have only 2mol CO coming from 1mol O2 If you make the first equation read 3mol CO, you will have to have 1.5mol O2. Now you can say that 1.5mol O2 are needed to produce 2mol Fe, or 0.75mol O2 are required to produce 1 mol Fe. Mathematically you would say: 1mol Fe produced by (3molCO/2molFe) * 1mol O2/2mol CO. 1mol Fe produced by (3*1)/(2*2) 3/4 0.75 mol O2 per mol Fe
The easiest way is to get both the equations to have commom molar quantities. You want to go from Oxygen to iron via CO In the second equation, 2mol Fe are produced from 3mol CO But in the first equation, you have only 2mol CO coming from 1mol O2 If you make the first equation read 3mol CO, you will have to have 1.5mol O2. Now you can say that 1.5mol O2 are needed to produce 2mol Fe, or 0.75mol O2 are required to produce 1 mol Fe. Mathematically you would say: 1mol Fe produced by (3molCO/2molFe) * 1mol O2/2mol CO. 1mol Fe produced by (3*1)/(2*2) 3/4 0.75 mol O2 per mol Fe
