In this situation, since we assume copper does not react, the reactants are only H +(aq) and Fe(s). Step 1: Write a balanced equation after determining the products and reactants. % error = | theoretical - experimental | / theoretical * 100% Check your result by calculating the molar mass of the molecular formula and comparing it to the experimentally determined mass.Įxperimentally determined mass = 120.056 g/mol Multiply the ratio from step 4 by the subscripts of the empirical formula to get the molecular formula.Ħ. If the answer is not close to a whole number, there was either an error in the calculation of the empirical formula or a large error in the determination of the molecular mass.ĥ. Step 2: Now click the button Balance to get the result. Since 3.9984 is very close to four, it is possible to safely round up and assume that there was a slight error in the experimentally determined molecular mass. The procedure to use the balancing chemical equations calculator is as follows: Step 1: Enter the chemical equation in the input field. In case the original equation was unbalanced, the field with this equation is highlighted in light pink. Divide the experimentally determined molecular mass by the mass of the empirical formula. This online Chemical Equation Balancer Calculator finds the stoichiometric coefficients to balance a given chemical equation, including equations with free electrons and electrically charged molecules (ions) as well as hydrated compounds. 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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