Input interpretation
![phenoxybenzamine hydrochloride | molar mass](../image_source/73dff8c883822ef93d4fa8add08cfa0c.png)
phenoxybenzamine hydrochloride | molar mass
Result
![Find the molar mass, M, for phenoxybenzamine hydrochloride: 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_18H_23Cl_2NO Use the chemical formula to count the number of atoms, N_i, for each element: | N_i C (carbon) | 18 Cl (chlorine) | 2 H (hydrogen) | 23 N (nitrogen) | 1 O (oxygen) | 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) C (carbon) | 18 | 12.011 Cl (chlorine) | 2 | 35.45 H (hydrogen) | 23 | 1.008 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: | | | N_i | m_i/g·mol^(-1) | mass/g·mol^(-1) C (carbon) | 18 | 12.011 | 18 × 12.011 = 216.198 Cl (chlorine) | 2 | 35.45 | 2 × 35.45 = 70.90 H (hydrogen) | 23 | 1.008 | 23 × 1.008 = 23.184 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 M = 216.198 g/mol + 70.90 g/mol + 23.184 g/mol + 14.007 g/mol + 15.999 g/mol = 340.29 g/mol](../image_source/a6a1810ab741e18047890d6600c706f0.png)
Find the molar mass, M, for phenoxybenzamine hydrochloride: 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_18H_23Cl_2NO Use the chemical formula to count the number of atoms, N_i, for each element: | N_i C (carbon) | 18 Cl (chlorine) | 2 H (hydrogen) | 23 N (nitrogen) | 1 O (oxygen) | 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) C (carbon) | 18 | 12.011 Cl (chlorine) | 2 | 35.45 H (hydrogen) | 23 | 1.008 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: | | | N_i | m_i/g·mol^(-1) | mass/g·mol^(-1) C (carbon) | 18 | 12.011 | 18 × 12.011 = 216.198 Cl (chlorine) | 2 | 35.45 | 2 × 35.45 = 70.90 H (hydrogen) | 23 | 1.008 | 23 × 1.008 = 23.184 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 M = 216.198 g/mol + 70.90 g/mol + 23.184 g/mol + 14.007 g/mol + 15.999 g/mol = 340.29 g/mol
Unit conversion
![0.3403 kg/mol (kilograms per mole)](../image_source/8bf4e99d3466e9b029713f60fc8b8616.png)
0.3403 kg/mol (kilograms per mole)
Comparisons
![≈ 0.47 × molar mass of fullerene ( ≈ 721 g/mol )](../image_source/20f17632e9f42bca8f12d7aff1fd9afd.png)
≈ 0.47 × molar mass of fullerene ( ≈ 721 g/mol )
![≈ 1.8 × molar mass of caffeine ( ≈ 194 g/mol )](../image_source/a8c01ae5011cb8baa25a83ed1d803e4e.png)
≈ 1.8 × molar mass of caffeine ( ≈ 194 g/mol )
![≈ 5.8 × molar mass of sodium chloride ( ≈ 58 g/mol )](../image_source/270e9e3d60dc6d379395f59315a2097c.png)
≈ 5.8 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
![Mass of a molecule m from m = M/N_A: | 5.7×10^-22 grams | 5.7×10^-25 kg (kilograms) | 340 u (unified atomic mass units) | 340 Da (daltons)](../image_source/e51d5ec466acb68f8c133fe677e7a35e.png)
Mass of a molecule m from m = M/N_A: | 5.7×10^-22 grams | 5.7×10^-25 kg (kilograms) | 340 u (unified atomic mass units) | 340 Da (daltons)
![Relative molecular mass M_r from M_r = M_u/M: | 340](../image_source/e4be59ee5f0179f09866005186c6d5f6.png)
Relative molecular mass M_r from M_r = M_u/M: | 340