Input interpretation
osmium(IV) fluoride | molar mass
Result
Find the molar mass, M, for osmium(IV) fluoride: M = sum _iN_im_i Plan: • Write the chemical formula and gather atomic masses from the periodic table. • Determine values for N_i and m_i using these items. • Finally, compute the mass. Write the chemical formula: OsF_4 Use the chemical formula, OsF_4, to count the number of atoms, N_i, for each element: | N_i F (fluorine) | 4 Os (osmium) | 1 Look up the atomic mass, m_i, in g·mol^(-1) for each element in the periodic table: | N_i | m_i/g·mol^(-1) F (fluorine) | 4 | 18.998403163 Os (osmium) | 1 | 190.23 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molar mass, M: Answer: | | | N_i | m_i/g·mol^(-1) | mass/g·mol^(-1) F (fluorine) | 4 | 18.998403163 | 4 × 18.998403163 = 75.993612652 Os (osmium) | 1 | 190.23 | 1 × 190.23 = 190.23 M = 75.993612652 g/mol + 190.23 g/mol = 266.22 g/mol
Unit conversion
0.26622 kg/mol (kilograms per mole)
Comparisons
≈ 0.37 × molar mass of fullerene ( ≈ 721 g/mol )
≈ 1.4 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 4.6 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 4.4×10^-22 grams | 4.4×10^-25 kg (kilograms) | 266 u (unified atomic mass units) | 266 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 266