The actual molar mass of butane is 58.1 g/mole.
Butane, with the molecular formula C4H10, is a common alkane gas used in lighters and portable stoves. Understanding its molar mass is crucial in various chemical calculations.
Calculating Molar Mass
Molar mass is the mass of one mole of a substance, and it is expressed in grams per mole (g/mol). Here's how the molar mass of butane is determined:
| Element | Number of Atoms | Atomic Mass (g/mol) | Total Mass (g/mol) |
|---|---|---|---|
| Carbon (C) | 4 | 12.01 | 48.04 |
| Hydrogen (H) | 10 | 1.008 | 10.08 |
| Total | 58.12 |
The molar mass is calculated by adding the total atomic masses of all elements in the formula. Based on the reference, the molar mass of butane is 58.1 g/mole.
Practical Applications
- Stoichiometry: The molar mass is essential for stoichiometric calculations, converting between grams and moles of butane in chemical reactions.
- Gas Laws: Used in calculations involving the Ideal Gas Law and other gas laws to relate pressure, volume, temperature, and the number of moles.
- Density: The molar mass helps calculate the density of butane gas.
Example Calculation
Let's say you need to determine how many moles are in 100 grams of butane. Using the molar mass:
Moles of Butane = Mass (g) / Molar Mass (g/mol)
Moles of Butane = 100 g / 58.1 g/mol
Moles of Butane ≈ 1.72 moles
This shows how crucial molar mass is for converting mass to moles and vice-versa.
