[chrisaltman]

Thanks again for all the help.

When 1.5173 g of an organic iron compound containing Fe, C, H, and O is burned in O₂, 2.838g of CO₂ and .8122g of H₂O are yielded. In a separate experiment to determine mass %, .3355 g of the compound yielded .0758g Fe₂O₃. What is the empirical formula of this compound?

Setting this equation up, I know to find the amount of moles of C and H in the first experiment, which are .06448607687 and .090167901914, respectively. From there, however, I can't figure it out. I know to find the mol of Fe in the second experiment, which is 9.49350045902*10^-4 mol. I know that the grams of C and H in the second experiment subtracted from the total value will give me the Fe and O masses, but how do I differentiate between the two? Any help will be greatly appreciated.

[DrCMS]

From the first part you can work out how much C and H are in sample 1
From the 2nd part you can work out how much Fe is in sample 2.
From the initial weight less the amount of C, H and Fe (corrected for sample weight 1) you can calculate the amount of O.
Turn those into moles and multiple/divide to get whole numbers gives you the empirical formula.

[chrisaltman]

From the first part you can work out how much C and H are in sample 1
From the 2nd part you can work out how much Fe is in sample 2.
From the initial weight less the amount of C, H and Fe (corrected for sample weight 1) you can calculate the amount of O.
Turn those into moles and multiple/divide to get whole numbers gives you the empirical formula.

Thanks. How do I correct the Fe weight from sample 2 to be appropriate for sample 1?