Input interpretation
nitric oxide | molar mass
Result
Find the molar mass, M, for nitric oxide: 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: NO Use the chemical formula to count the number of atoms, N_i, for each element: | number of atoms N (nitrogen) | 1 O (oxygen) | 1 Look up the atomic mass, m_i, in g·mol^(-1) for each element in the periodic table: | number of atoms | atomic mass/g·mol^(-1) N (nitrogen) | 1 | 14.007 O (oxygen) | 1 | 15.999 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molar mass, M: Answer: | | | number of atoms | atomic mass/g·mol^(-1) | mass/g·mol^(-1) N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 M = 14.007 g/mol + 15.999 g/mol = 30.006 g/mol
Unit conversion
0.030006 kg/mol (kilograms per mole)
Comparisons
≈ ( 0.15 ≈ 1/6 ) × molar mass of caffeine (≈ 194 g/mol )
≈ 0.51 × molar mass of sodium chloride (≈ 58 g/mol )
≈ 1.7 × molar mass of water (≈ 18 g/mol )
Corresponding quantities
Mass of a molecule m from m = M/N_A: | 5×10^-23 grams | 5×10^-26 kg (kilograms) | 30 u (unified atomic mass units) | 30 Da (daltons)
Relative molecular mass M_r from M_r = M_u/M: | 30