![]() ![]() (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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