Input interpretation
1-chloro-1, 2, 2-trifluorocyclobutane | molar mass
Result
Find the molar mass, M, for 1-chloro-1, 2, 2-trifluorocyclobutane: 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_4H_4ClF_3 Use the chemical formula, C_4H_4ClF_3, to count the number of atoms, N_i, for each element: | N_i C (carbon) | 4 Cl (chlorine) | 1 F (fluorine) | 3 H (hydrogen) | 4 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) | 4 | 12.011 Cl (chlorine) | 1 | 35.45 F (fluorine) | 3 | 18.998403163 H (hydrogen) | 4 | 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) | 4 | 12.011 | 4 × 12.011 = 48.044 Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 F (fluorine) | 3 | 18.998403163 | 3 × 18.998403163 = 56.995209489 H (hydrogen) | 4 | 1.008 | 4 × 1.008 = 4.032 M = 48.044 g/mol + 35.45 g/mol + 56.995209489 g/mol + 4.032 g/mol = 144.52 g/mol
Unit conversion
0.14452 kg/mol (kilograms per mole)
Comparisons
≈ ( 0.2 ≈ 1/5 ) × molar mass of fullerene ( ≈ 721 g/mol )
≈ 0.74 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 2.5 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 2.4×10^-22 grams | 2.4×10^-25 kg (kilograms) | 145 u (unified atomic mass units) | 145 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 145