mass fractions of sulfuryl chloride fluoride

sulfuryl chloride fluoride | elemental composition

Find the elemental composition for sulfuryl chloride fluoride in terms of the atom and mass percents: atom percent = N_i/N_atoms × 100% mass percent = (N_im_i)/m × 100% Plan: • Write the chemical formula and gather atomic masses from the periodic table. • Determine values for N_i, m_i, N_atoms and m using these items. • Finally, compute the percents and check the results. Write the chemical formula: SO_2ClF Use the chemical formula, SO_2ClF, to count the number of atoms, N_i, for each element and find the total number of atoms, N_atoms: | number of atoms Cl (chlorine) | 1 F (fluorine) | 1 O (oxygen) | 2 S (sulfur) | 1 N_atoms = 1 + 1 + 2 + 1 = 5 Divide each N_i by N_atoms to calculate atom fractions. Then use the property that atom fractions must sum to one to check the work: | number of atoms | atom fraction Cl (chlorine) | 1 | 1/5 F (fluorine) | 1 | 1/5 O (oxygen) | 2 | 2/5 S (sulfur) | 1 | 1/5 Check: 1/5 + 1/5 + 2/5 + 1/5 = 1 Compute atom percents using the atom fractions: | number of atoms | atom percent Cl (chlorine) | 1 | 1/5 × 100% = 20.0% F (fluorine) | 1 | 1/5 × 100% = 20.0% O (oxygen) | 2 | 2/5 × 100% = 40.0% S (sulfur) | 1 | 1/5 × 100% = 20.0% Look up the atomic mass, m_i, in unified atomic mass units, u, for each element in the periodic table: | number of atoms | atom percent | atomic mass/u Cl (chlorine) | 1 | 20.0% | 35.45 F (fluorine) | 1 | 20.0% | 18.998403163 O (oxygen) | 2 | 40.0% | 15.999 S (sulfur) | 1 | 20.0% | 32.06 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molecular mass, m: | number of atoms | atom percent | atomic mass/u | mass/u Cl (chlorine) | 1 | 20.0% | 35.45 | 1 × 35.45 = 35.45 F (fluorine) | 1 | 20.0% | 18.998403163 | 1 × 18.998403163 = 18.998403163 O (oxygen) | 2 | 40.0% | 15.999 | 2 × 15.999 = 31.998 S (sulfur) | 1 | 20.0% | 32.06 | 1 × 32.06 = 32.06 m = 35.45 u + 18.998403163 u + 31.998 u + 32.06 u = 118.506403163 u Divide the mass for each element by m to calculate mass fractions. Then use the property that mass fractions must sum to one to check the work: | number of atoms | atom percent | mass fraction Cl (chlorine) | 1 | 20.0% | 35.45/118.506403163 F (fluorine) | 1 | 20.0% | 18.998403163/118.506403163 O (oxygen) | 2 | 40.0% | 31.998/118.506403163 S (sulfur) | 1 | 20.0% | 32.06/118.506403163 Check: 35.45/118.506403163 + 18.998403163/118.506403163 + 31.998/118.506403163 + 32.06/118.506403163 = 1 Compute mass percents using the mass fractions: Answer: | | | number of atoms | atom percent | mass percent Cl (chlorine) | 1 | 20.0% | 35.45/118.506403163 × 100% = 29.91% F (fluorine) | 1 | 20.0% | 18.998403163/118.506403163 × 100% = 16.03% O (oxygen) | 2 | 40.0% | 31.998/118.506403163 × 100% = 27.00% S (sulfur) | 1 | 20.0% | 32.06/118.506403163 × 100% = 27.05%

Mass fraction pie chart