Input interpretation
![hydroxylamine perchlorate | molar mass](../image_source/fc109301e53e66c75355295aec9a6ad5.png)
hydroxylamine perchlorate | molar mass
Result
![Find the molar mass, M, for hydroxylamine perchlorate: 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: H_2NOH·HClO_4 Use the chemical formula, H_2NOH·HClO_4, to count the number of atoms, N_i, for each element: | N_i Cl (chlorine) | 1 H (hydrogen) | 4 N (nitrogen) | 1 O (oxygen) | 5 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 H (hydrogen) | 4 | 1.008 N (nitrogen) | 1 | 14.007 O (oxygen) | 5 | 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) Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 H (hydrogen) | 4 | 1.008 | 4 × 1.008 = 4.032 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 5 | 15.999 | 5 × 15.999 = 79.995 M = 35.45 g/mol + 4.032 g/mol + 14.007 g/mol + 79.995 g/mol = 133.48 g/mol](../image_source/254687a1af53dac2289821b32d2e516a.png)
Find the molar mass, M, for hydroxylamine perchlorate: 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: H_2NOH·HClO_4 Use the chemical formula, H_2NOH·HClO_4, to count the number of atoms, N_i, for each element: | N_i Cl (chlorine) | 1 H (hydrogen) | 4 N (nitrogen) | 1 O (oxygen) | 5 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 H (hydrogen) | 4 | 1.008 N (nitrogen) | 1 | 14.007 O (oxygen) | 5 | 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) Cl (chlorine) | 1 | 35.45 | 1 × 35.45 = 35.45 H (hydrogen) | 4 | 1.008 | 4 × 1.008 = 4.032 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 5 | 15.999 | 5 × 15.999 = 79.995 M = 35.45 g/mol + 4.032 g/mol + 14.007 g/mol + 79.995 g/mol = 133.48 g/mol
Unit conversion
![0.1335 kg/mol (kilograms per mole)](../image_source/add77ef1f427066d13841630de722de2.png)
0.1335 kg/mol (kilograms per mole)
Comparisons
![≈ ( 0.19 ≈ 1/5 ) × molar mass of fullerene ( ≈ 721 g/mol )](../image_source/37e9ccf4dda395e00b6fb1eaedc71ccf.png)
≈ ( 0.19 ≈ 1/5 ) × molar mass of fullerene ( ≈ 721 g/mol )
![≈ 0.69 × molar mass of caffeine ( ≈ 194 g/mol )](../image_source/69b1fb31ba0293956063c032fa06c8c0.png)
≈ 0.69 × molar mass of caffeine ( ≈ 194 g/mol )
![≈ 2.3 × molar mass of sodium chloride ( ≈ 58 g/mol )](../image_source/06d3e56cc74f638ad7134c1a9f0d387a.png)
≈ 2.3 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
![Mass of a molecule m from m = M/N_A: | 2.2×10^-22 grams | 2.2×10^-25 kg (kilograms) | 133 u (unified atomic mass units) | 133 Da (daltons)](../image_source/c76f6e622c8826a210957e7efcd6928a.png)
Mass of a molecule m from m = M/N_A: | 2.2×10^-22 grams | 2.2×10^-25 kg (kilograms) | 133 u (unified atomic mass units) | 133 Da (daltons)
![Relative molecular mass M_r from M_r = M_u/M: | 133](../image_source/d86a02b76687d22fed666c3cfbc3ec05.png)
Relative molecular mass M_r from M_r = M_u/M: | 133