Input interpretation
potassium hexacyanoferrate(III) | molar mass
Result
Find the molar mass, M, for potassium hexacyanoferrate(III): 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: K_3Fe(CN)_6 Use the chemical formula, K_3Fe(CN)_6, to count the number of atoms, N_i, for each element: | N_i C (carbon) | 6 Fe (iron) | 1 K (potassium) | 3 N (nitrogen) | 6 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) C (carbon) | 6 | 12.011 Fe (iron) | 1 | 55.845 K (potassium) | 3 | 39.0983 N (nitrogen) | 6 | 14.007 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) C (carbon) | 6 | 12.011 | 6 × 12.011 = 72.066 Fe (iron) | 1 | 55.845 | 1 × 55.845 = 55.845 K (potassium) | 3 | 39.0983 | 3 × 39.0983 = 117.2949 N (nitrogen) | 6 | 14.007 | 6 × 14.007 = 84.042 M = 72.066 g/mol + 55.845 g/mol + 117.2949 g/mol + 84.042 g/mol = 329.248 g/mol
Unit conversion
0.32925 kg/mol (kilograms per mole)
Comparisons
≈ 0.46 × molar mass of fullerene ( ≈ 721 g/mol )
≈ 1.7 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 5.6 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 5.5×10^-22 grams | 5.5×10^-25 kg (kilograms) | 329 u (unified atomic mass units) | 329 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 329