Input interpretation
aluminum oleate | molar mass
Result
Find the molar mass, M, for aluminum oleate: 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: C_54H_99AlO_6 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i Al (aluminum) | 1 C (carbon) | 54 H (hydrogen) | 99 O (oxygen) | 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) Al (aluminum) | 1 | 26.9815385 C (carbon) | 54 | 12.011 H (hydrogen) | 99 | 1.008 O (oxygen) | 6 | 15.999 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) Al (aluminum) | 1 | 26.9815385 | 1 × 26.9815385 = 26.9815385 C (carbon) | 54 | 12.011 | 54 × 12.011 = 648.594 H (hydrogen) | 99 | 1.008 | 99 × 1.008 = 99.792 O (oxygen) | 6 | 15.999 | 6 × 15.999 = 95.994 M = 26.9815385 g/mol + 648.594 g/mol + 99.792 g/mol + 95.994 g/mol = 871.362 g/mol
Unit conversion
0.8714 kg/mol (kilograms per mole)
Comparisons
≈ 1.2 × molar mass of fullerene ( ≈ 721 g/mol )
≈ 4.5 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 15 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 1.4×10^-21 grams | 1.4×10^-24 kg (kilograms) | 871 u (unified atomic mass units) | 871 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 871