Input interpretation
![4 methylenedioxyphenethylamine hydrochloride | molar mass](../image_source/270e8d7c45ab745bf21083d6d719d351.png)
4 methylenedioxyphenethylamine hydrochloride | molar mass
Result
![Find the molar mass, M, for 4 methylenedioxyphenethylamine 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_9H_12ClNO_2 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i Cl (chlorine) | 1 C (carbon) | 9 O (oxygen) | 2 N (nitrogen) | 1 H (hydrogen) | 12 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) Cl (chlorine) | 1 | 35.45 C (carbon) | 9 | 12.011 O (oxygen) | 2 | 15.999 N (nitrogen) | 1 | 14.007 H (hydrogen) | 12 | 1.008 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) Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 C (carbon) | 9 | 12.011 | 9 × 12.011 = 108.099 O (oxygen) | 2 | 15.999 | 2 × 15.999 = 31.998 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 H (hydrogen) | 12 | 1.008 | 12 × 1.008 = 12.096 M = 35.45 g/mol + 108.099 g/mol + 31.998 g/mol + 14.007 g/mol + 12.096 g/mol = 201.65 g/mol](../image_source/e19c4549da10c7f0daf0d4144a55f7b0.png)
Find the molar mass, M, for 4 methylenedioxyphenethylamine 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_9H_12ClNO_2 Use the chemical formula to count the number of atoms, N_i, for each element: | N_i Cl (chlorine) | 1 C (carbon) | 9 O (oxygen) | 2 N (nitrogen) | 1 H (hydrogen) | 12 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) Cl (chlorine) | 1 | 35.45 C (carbon) | 9 | 12.011 O (oxygen) | 2 | 15.999 N (nitrogen) | 1 | 14.007 H (hydrogen) | 12 | 1.008 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) Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 C (carbon) | 9 | 12.011 | 9 × 12.011 = 108.099 O (oxygen) | 2 | 15.999 | 2 × 15.999 = 31.998 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 H (hydrogen) | 12 | 1.008 | 12 × 1.008 = 12.096 M = 35.45 g/mol + 108.099 g/mol + 31.998 g/mol + 14.007 g/mol + 12.096 g/mol = 201.65 g/mol
Unit conversion
![0.2017 kg/mol (kilograms per mole)](../image_source/9aec8a6c4eb48e8e29640bfce481fecb.png)
0.2017 kg/mol (kilograms per mole)
Comparisons
![≈ 0.28 × molar mass of fullerene ( ≈ 721 g/mol )](../image_source/273791324764978ef2aaaa0caf2e5d32.png)
≈ 0.28 × molar mass of fullerene ( ≈ 721 g/mol )
![≈ molar mass of caffeine ( ≈ 194 g/mol )](../image_source/a58151ef86b01cacdb44f999cb777a21.png)
≈ molar mass of caffeine ( ≈ 194 g/mol )
![≈ 3.5 × molar mass of sodium chloride ( ≈ 58 g/mol )](../image_source/cef436ee0e4b025d0a2aa5c72f295e7d.png)
≈ 3.5 × 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) | 202 u (unified atomic mass units) | 202 Da (daltons)](../image_source/04dd6642e291f936f4480970beecd32f.png)
Mass of a molecule m from m = M/N_A: | 3.3×10^-22 grams | 3.3×10^-25 kg (kilograms) | 202 u (unified atomic mass units) | 202 Da (daltons)
![Relative molecular mass M_r from M_r = M_u/M: | 202](../image_source/6244611502e08046682d5dc7755dae09.png)
Relative molecular mass M_r from M_r = M_u/M: | 202