Input interpretation
octafluorocyclobutane | molar mass
Result
Find the molar mass, M, for octafluorocyclobutane: 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_4F_8 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i C (carbon) | 4 F (fluorine) | 8 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 F (fluorine) | 8 | 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) C (carbon) | 4 | 12.011 | 4 × 12.011 = 48.044 F (fluorine) | 8 | 18.998403163 | 8 × 18.998403163 = 151.987225304 M = 48.044 g/mol + 151.987225304 g/mol = 200.031 g/mol
Unit conversion
0.200031 kg/mol (kilograms per mole)
Comparisons
≈ 0.28 × molar mass of fullerene ( ≈ 721 g/mol )
≈ molar mass of caffeine ( ≈ 194 g/mol )
≈ 3.4 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 3.3×10^-22 grams | 3.3×10^-25 kg (kilograms) | 200 u (unified atomic mass units) | 200 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 200