a sample contains only Fe2O3 and AL2O3 which weighs 0.5622 grams. It is heated with H2, reducing Fe2O3 to Fe, Leaving the AL2O3 unchanged. the mixture now has a mass of .4582 grams. Calculate the percentage of Al in the sample.

Question

a  sample contains only Fe2O3 and AL2O3 which weighs 0.5622 grams. It is heated with H2, reducing Fe2O3 to Fe, Leaving the AL2O3 unchanged. the mixture now has a mass of .4582 grams. Calculate the percentage of Al in the sample.

btaylor · Answer

to make it easier, lets multiply all the numbers by 1000
5622 - 4582 = 1040 g O --> 65 mol O --> 43.3 mol Fe --> 2420 g Fe. So 
5622 - 2420 = 3202 g Al2O3. If you want % of Al2O3, it is 57%
in Al2O3, Al is 52.9%. So 0.529 x 3202 = 1693.9 g Al
1693.9/5622 = 30.1% Al

anonymous · Answer

thanks BTaylor my answer was just up ot the conversion of Fe.. thanks for the direction i can go through my anwers.. i know the principles. but having a hard time executing to the problem..

btaylor · Answer

yw