Input interpretation
![ammonium bromate | molar mass](../image_source/d258e6165e89f0f7cd3b8ff21e7e1a75.png)
ammonium bromate | molar mass
Result
![Find the molar mass, M, for ammonium bromate: 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: BrH_4NO_3 Use the chemical formula, BrH_4NO_3, to count the number of atoms, N_i, for each element: | N_i Br (bromine) | 1 H (hydrogen) | 4 N (nitrogen) | 1 O (oxygen) | 3 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) Br (bromine) | 1 | 79.904 H (hydrogen) | 4 | 1.008 N (nitrogen) | 1 | 14.007 O (oxygen) | 3 | 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) Br (bromine) | 1 | 79.904 | 1 × 79.904 = 79.904 H (hydrogen) | 4 | 1.008 | 4 × 1.008 = 4.032 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 3 | 15.999 | 3 × 15.999 = 47.997 M = 79.904 g/mol + 4.032 g/mol + 14.007 g/mol + 47.997 g/mol = 145.940 g/mol](../image_source/7ea448b6bd127237a9c2e463688ffe92.png)
Find the molar mass, M, for ammonium bromate: 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: BrH_4NO_3 Use the chemical formula, BrH_4NO_3, to count the number of atoms, N_i, for each element: | N_i Br (bromine) | 1 H (hydrogen) | 4 N (nitrogen) | 1 O (oxygen) | 3 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) Br (bromine) | 1 | 79.904 H (hydrogen) | 4 | 1.008 N (nitrogen) | 1 | 14.007 O (oxygen) | 3 | 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) Br (bromine) | 1 | 79.904 | 1 × 79.904 = 79.904 H (hydrogen) | 4 | 1.008 | 4 × 1.008 = 4.032 N (nitrogen) | 1 | 14.007 | 1 × 14.007 = 14.007 O (oxygen) | 3 | 15.999 | 3 × 15.999 = 47.997 M = 79.904 g/mol + 4.032 g/mol + 14.007 g/mol + 47.997 g/mol = 145.940 g/mol
Unit conversion
![0.14594 kg/mol (kilograms per mole)](../image_source/73377e63179f7e97eeb1e62de01f774a.png)
0.14594 kg/mol (kilograms per mole)
Comparisons
![≈ ( 0.2 ≈ 1/5 ) × molar mass of fullerene ( ≈ 721 g/mol )](../image_source/a69acce9bcfa0c86e4e3ddfae616651e.png)
≈ ( 0.2 ≈ 1/5 ) × molar mass of fullerene ( ≈ 721 g/mol )
![≈ 0.75 × molar mass of caffeine ( ≈ 194 g/mol )](../image_source/3ef2c5e86a5098f3d2ab92c949f8b6be.png)
≈ 0.75 × molar mass of caffeine ( ≈ 194 g/mol )
![≈ 2.5 × molar mass of sodium chloride ( ≈ 58 g/mol )](../image_source/a42dd95fa7bfca009a36e7be21cd0923.png)
≈ 2.5 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
![Mass of a molecule m from m = M/N_A: | 2.4×10^-22 grams | 2.4×10^-25 kg (kilograms) | 146 u (unified atomic mass units) | 146 Da (daltons)](../image_source/378e3e4132e7dea901d3f45a19e30663.png)
Mass of a molecule m from m = M/N_A: | 2.4×10^-22 grams | 2.4×10^-25 kg (kilograms) | 146 u (unified atomic mass units) | 146 Da (daltons)
![Relative molecular mass M_r from M_r = M_u/M: | 146](../image_source/34710f4de0c34f109b34a9d104895eaf.png)
Relative molecular mass M_r from M_r = M_u/M: | 146