Input interpretation
acetyl fluoride | molar mass
Result
Find the molar mass, M, for acetyl 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: CH_3COF Use the chemical formula to count the number of atoms, N_i, for each element: | N_i C (carbon) | 2 F (fluorine) | 1 H (hydrogen) | 3 O (oxygen) | 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) C (carbon) | 2 | 12.011 F (fluorine) | 1 | 18.998403163 H (hydrogen) | 3 | 1.008 O (oxygen) | 1 | 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) C (carbon) | 2 | 12.011 | 2 × 12.011 = 24.022 F (fluorine) | 1 | 18.998403163 | 1 × 18.998403163 = 18.998403163 H (hydrogen) | 3 | 1.008 | 3 × 1.008 = 3.024 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 M = 24.022 g/mol + 18.998403163 g/mol + 3.024 g/mol + 15.999 g/mol = 62.043 g/mol
Unit conversion
0.062043 kg/mol (kilograms per mole)
Comparisons
≈ ( 0.086 ≈ 1/12 ) × molar mass of fullerene ( ≈ 721 g/mol )
≈ 0.32 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 1.1 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 1×10^-22 grams | 1×10^-25 kg (kilograms) | 62 u (unified atomic mass units) | 62 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 62