Input interpretation
iodine azide | molar mass
Result
Find the molar mass, M, for iodine azide: 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: IN_3 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i I (iodine) | 1 N (nitrogen) | 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) I (iodine) | 1 | 126.90447 N (nitrogen) | 3 | 14.007 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) I (iodine) | 1 | 126.90447 | 1 × 126.90447 = 126.90447 N (nitrogen) | 3 | 14.007 | 3 × 14.007 = 42.021 M = 126.90447 g/mol + 42.021 g/mol = 168.925 g/mol
Unit conversion
0.168925 kg/mol (kilograms per mole)
Comparisons
≈ ( 0.23 ≈ 1/4 ) × molar mass of fullerene ( ≈ 721 g/mol )
≈ 0.87 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 2.9 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 2.8×10^-22 grams | 2.8×10^-25 kg (kilograms) | 169 u (unified atomic mass units) | 169 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 169