Input interpretation
ammonium sulfate nitrate | molar mass
Result
Find the molar mass, M, for ammonium sulfate nitrate: 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: (NH_4)_3SO_4NO_3 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i H (hydrogen) | 12 N (nitrogen) | 4 O (oxygen) | 7 S (sulfur) | 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) H (hydrogen) | 12 | 1.008 N (nitrogen) | 4 | 14.007 O (oxygen) | 7 | 15.999 S (sulfur) | 1 | 32.06 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) H (hydrogen) | 12 | 1.008 | 12 × 1.008 = 12.096 N (nitrogen) | 4 | 14.007 | 4 × 14.007 = 56.028 O (oxygen) | 7 | 15.999 | 7 × 15.999 = 111.993 S (sulfur) | 1 | 32.06 | 1 × 32.06 = 32.06 M = 12.096 g/mol + 56.028 g/mol + 111.993 g/mol + 32.06 g/mol = 212.18 g/mol
Unit conversion
0.21218 kg/mol (kilograms per mole)
Comparisons
≈ 0.29 × molar mass of fullerene ( ≈ 721 g/mol )
≈ 1.1 × molar mass of caffeine ( ≈ 194 g/mol )
≈ 3.6 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 3.5×10^-22 grams | 3.5×10^-25 kg (kilograms) | 212 u (unified atomic mass units) | 212 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 212