![]() Determine the molecular mass experimentally. In the example above, it was determined that the unknown molecule had an empirical formula of CH 2O.ġ. (1/0.0332)(0.0333mol C : 0.0665mol H : 0.0332 mol O) => 1mol C: 2 mol H: 1 mol Oįrom this ratio, the empirical formula is calculated to be CH 2O. (0.0666mol O + 0.0332 mol O) - 0.0666mol O = 0.0332 mol OĬonstruct a mole ratio for C, H, and O in the unknown and divide by the smallest number. ![]() With this we can use the difference of the final mass of products and initial mass of the unknown organic molecule to determine the mass of the O 2 reactant.Ġ.333mol CO 2(44.0098g CO 2/ 1mol CO 2) = 1.466g CO 2ġ.466g CO 2 + 0.599g H 2O - 1.000g unknown organic = 1.065g O 2ġ.065g O 2( 1mol O 2/ 31.9988g O 2)( 2mol O/ 1mol O 2) = 0.0666mol O Using the Law of Conservation, we know that the mass before a reaction must equal the mass after a reaction. This will give you the number of moles from both the unknown organic molecule and the O 2 so you must subtract the moles of oxygen transferred from the O 2.Ġ.0333mol CO 2 ( 2mol O/ 1mol CO 2) = 0.0666 mol OĠ.599g H 2O ( 1mol H 2O/18.01528 g H 2O)( 1mol O/ 1mol H 2O) = 0.0332 mol O ![]() Since all the moles of C and H in CO 2 and H 2O, respectively have to have came from the 1 gram sample of unknown, start by calculating how many moles of each element were present in the unknown sample.Ġ.0333mol CO 2 ( 1mol C/ 1mol CO 2) = 0.0333mol C in unknownĠ.599g H 2O ( 1mol H 2O/ 18.01528g H 2O)( 2mol H/ 1mol H 2O) = 0.0665 mol H in unknownĬalculate the final moles of oxygen by taking the sum of the moles of oxygen in CO 2 and H 2O.
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