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I think you should find the empirical formula first by converting each atom into moles. % of atom = mass of atom in the compound mass of atom x (1/molar mass of atom) = # number of moles then divide each mole by the smallest mole number.. This will give you the pseudo chemical formula of the compound. After you finish this part, I'll tell you what's the next step.
15.81 g of Carbon convert it to moles. you may need to use the periodic table. Molar mass of carbon is approx 12 g/mol 15.81 g C (1 mol C /12 g C) g will get cancelled, so you'll left with 15.81/12 mol of C Use calc to simplify Do the same thing for O, and H
what did you get for the oxygen?
Oh sorry lol, I thought it is oxygen So you are right. Empirical formula would be \(\sf C_2HI\) The last step you have to do it to find the molar mass of this compound using the empirical formula that you found. Then, divide the given molar mass by the molar mass you calculated from the empirical formula. The quotient will serve as the factor to gain the molecular formula.
C = 2 x 12 H = 1 I = 127 add these, what will you get?
yes, then divide the given molar mass(455.7) to that calculated molar mass(152)
yes so 3 will be the factor|dw:1443060372787:dw|
Just a recap from @owlet 's instructions to mine. For future reference: 1. Assume a 100g sample: % of atom = mass of atom in the compound 2. Convert masses to moles: given mass (1/molar mass) 3. Calculate mole ratio: Dividing the smallest mole from step 2 4. Write the empirical formula 5. Calculate the Molar Mass of the compound from the empirical chemical formula 6. Divide the given molar mass by the molar mass calculated from step 5 7. The quotient will be the factor, which will be used to write the molecular mass :)