Fill in the details and click Calculate to see your results.
The mole fraction of a component is its share of the total number of moles in a mixture. It has no unit and does not change with temperature. It is used in Raoult's law and for partial pressures of gases.
Enter the mass and molar mass of each component. The calculator converts both to moles and gives the mole fraction and mole percent of each.
| Mass of component A | 46 g |
| Molar mass of A | 46.07 g/mol |
| Mass of component B | 54 g |
| Molar mass of B | 18.02 g/mol |
| Mole fraction of A (χA) | 0.249879 |
| Mole fraction of B (χB) | 0.750121 |
| Mole percent of A | 24.99% |
| Moles of A (mol) | 0.998524 |
| Moles of B (mol) | 2.9975 |
Ethanol's mole fraction is 0.249879, even though it is 46% of the mass.
Try this example →| Mass of component A | 50 g |
| Molar mass of A | 32.04 g/mol |
| Mass of component B | 50 g |
| Molar mass of B | 18.02 g/mol |
| Mole fraction of A (χA) | 0.35989 |
| Mole fraction of B (χB) | 0.64011 |
| Mole percent of A | 35.99% |
| Moles of A (mol) | 1.56045 |
| Moles of B (mol) | 2.77546 |
Methanol's mole fraction is 0.35989.
Try this example →For an ideal solution the partial vapour pressure of each component is its mole fraction times the vapour pressure of the pure component: p_A = χA × p°A.
The number of moles of one component divided by the total number of moles in the mixture.
No, it is a ratio.
Exactly 1.
No, because it depends only on amounts, not volume.