Input interpretation
1, 1, 3-trichlorotrifluoroacetone | molar mass
Result
Find the molar mass, M, for 1, 1, 3-trichlorotrifluoroacetone: 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_3Cl_3F_3O Use the chemical formula to count the number of atoms, N_i, for each element: | N_i Cl (chlorine) | 3 C (carbon) | 3 O (oxygen) | 1 F (fluorine) | 3 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) Cl (chlorine) | 3 | 35.45 C (carbon) | 3 | 12.011 O (oxygen) | 1 | 15.999 F (fluorine) | 3 | 18.998403163 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) Cl (chlorine) | 3 | 35.45 | 3 × 35.45 = 106.35 C (carbon) | 3 | 12.011 | 3 × 12.011 = 36.033 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 F (fluorine) | 3 | 18.998403163 | 3 × 18.998403163 = 56.995209489 M = 106.35 g/mol + 36.033 g/mol + 15.999 g/mol + 56.995209489 g/mol = 215.38 g/mol
Unit conversion
0.2154 kg/mol (kilograms per mole)
Comparisons
≈ 0.3 × molar mass of fullerene ( ≈ 721 g/mol )
≈ 1.1 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 3.7 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 3.6×10^-22 grams | 3.6×10^-25 kg (kilograms) | 215 u (unified atomic mass units) | 215 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 215