Input interpretation
![vanadium(II) oxide | molar mass](../image_source/d8d74822d502f2313993c784583652b3.png)
vanadium(II) oxide | molar mass
Result
![Find the molar mass, M, for vanadium(II) 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: OV Use the chemical formula to count the number of atoms, N_i, for each element: | N_i O (oxygen) | 1 V (vanadium) | 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) O (oxygen) | 1 | 15.999 V (vanadium) | 1 | 50.9415 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) O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 V (vanadium) | 1 | 50.9415 | 1 × 50.9415 = 50.9415 M = 15.999 g/mol + 50.9415 g/mol = 66.941 g/mol](../image_source/f0a1c0321c8d6d1c7e6b354f233c8cbd.png)
Find the molar mass, M, for vanadium(II) 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: OV Use the chemical formula to count the number of atoms, N_i, for each element: | N_i O (oxygen) | 1 V (vanadium) | 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) O (oxygen) | 1 | 15.999 V (vanadium) | 1 | 50.9415 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) O (oxygen) | 1 | 15.999 | 1 × 15.999 = 15.999 V (vanadium) | 1 | 50.9415 | 1 × 50.9415 = 50.9415 M = 15.999 g/mol + 50.9415 g/mol = 66.941 g/mol
Unit conversion
![0.066941 kg/mol (kilograms per mole)](../image_source/f19d6a3b629caa9f0d9e86309a5398ca.png)
0.066941 kg/mol (kilograms per mole)
Comparisons
![≈ ( 0.093 ≈ 1/11 ) × molar mass of fullerene ( ≈ 721 g/mol )](../image_source/fb246dee0d373b122daabdee5367c427.png)
≈ ( 0.093 ≈ 1/11 ) × molar mass of fullerene ( ≈ 721 g/mol )
![≈ 0.34 × molar mass of caffeine ( ≈ 194 g/mol )](../image_source/fe90861af69bf28a4a0d52f27baa8046.png)
≈ 0.34 × molar mass of caffeine ( ≈ 194 g/mol )
![≈ 1.1 × molar mass of sodium chloride ( ≈ 58 g/mol )](../image_source/523ce41b7e009121ba521f6009b7be3c.png)
≈ 1.1 × molar mass of sodium chloride ( ≈ 58 g/mol )
Corresponding quantities
![Mass of a molecule m from m = M/N_A: | 1.1×10^-22 grams | 1.1×10^-25 kg (kilograms) | 67 u (unified atomic mass units) | 67 Da (daltons)](../image_source/f89d8c897b973100a07919573480eb21.png)
Mass of a molecule m from m = M/N_A: | 1.1×10^-22 grams | 1.1×10^-25 kg (kilograms) | 67 u (unified atomic mass units) | 67 Da (daltons)
![Relative molecular mass M_r from M_r = M_u/M: | 67](../image_source/b7b9acd4c7a8b3e063a02a41aae6af59.png)
Relative molecular mass M_r from M_r = M_u/M: | 67