Input interpretation
1-chloro-2, 2, 2-trifluoroethane | molar mass
Result
Find the molar mass, M, for 1-chloro-2, 2, 2-trifluoroethane: 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_2H_2ClF_3 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i C (carbon) | 2 Cl (chlorine) | 1 F (fluorine) | 3 H (hydrogen) | 2 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 Cl (chlorine) | 1 | 35.45 F (fluorine) | 3 | 18.998403163 H (hydrogen) | 2 | 1.008 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 Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 F (fluorine) | 3 | 18.998403163 | 3 × 18.998403163 = 56.995209489 H (hydrogen) | 2 | 1.008 | 2 × 1.008 = 2.016 M = 24.022 g/mol + 35.45 g/mol + 56.995209489 g/mol + 2.016 g/mol = 118.48 g/mol
Unit conversion
0.1185 kg/mol (kilograms per mole)
Comparisons
≈ ( 0.16 ≈ 1/6 ) × molar mass of fullerene ( ≈ 721 g/mol )
≈ 0.61 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 2 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 2×10^-22 grams | 2×10^-25 kg (kilograms) | 118 u (unified atomic mass units) | 118 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 118