Input interpretation
1, 1, 1-trifluoro-2-phenyl-3-buten-2-ol | molar mass
Result
Find the molar mass, M, for 1, 1, 1-trifluoro-2-phenyl-3-buten-2-ol: 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_2=CHC(CF_3)(OH)C_6H_5 Use the chemical formula, CH_2=CHC(CF_3)(OH)C_6H_5, to count the number of atoms, N_i, for each element: | N_i C (carbon) | 10 F (fluorine) | 3 H (hydrogen) | 9 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) | 10 | 12.011 F (fluorine) | 3 | 18.998403163 H (hydrogen) | 9 | 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) | 10 | 12.011 | 10 × 12.011 = 120.110 F (fluorine) | 3 | 18.998403163 | 3 × 18.998403163 = 56.995209489 H (hydrogen) | 9 | 1.008 | 9 × 1.008 = 9.072 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 M = 120.110 g/mol + 56.995209489 g/mol + 9.072 g/mol + 15.999 g/mol = 202.176 g/mol
Unit conversion
0.20218 kg/mol (kilograms per mole)
Comparisons
≈ 0.28 × molar mass of fullerene ( ≈ 721 g/mol )
≈ molar mass of caffeine ( ≈ 194 g/mol )
≈ 3.5 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 3.4×10^-22 grams | 3.4×10^-25 kg (kilograms) | 202 u (unified atomic mass units) | 202 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 202