Butane Molar Mass Calculator

Butane Molar Mass Result

58.124 g/mol

Formula: C₄H₁₀ · Total atoms: 14

Mass58.124 g

Moles1 mol

Molecules6.02214076 × 10²³

Selected precision3 decimals

Known quantity Choose the quantity you already know.

Quantity value Enter a nonnegative numeric value.

Mass unit Mass is converted to grams internally.

Display precision Precision changes displayed rounding only.

Carbon atomic mass Default standard atomic mass value.

Hydrogen atomic mass Default standard atomic mass value.

Calculation steps

Carbon contribution: 4 × 12.011 = 48.044 g/mol.
Hydrogen contribution: 10 × 1.008 = 10.080 g/mol.
Total molar mass: 48.044 + 10.080 = 58.124 g/mol.
Mass to moles: 58.124 ÷ 58.124 = 1 mol.
Moles to molecules: 1 × 6.02214076 × 10²³.

Formula Used

Butane formula: C₄H₁₀

M = (4 × atomic mass of C) + (10 × atomic mass of H)

Moles = mass in grams ÷ molar mass

Molecules = moles × 6.02214076 × 10^23

How to Use This Calculator

Select mass, moles, or molecules as your known quantity. Enter the value and choose any needed mass unit. Select the displayed precision before calculating the remaining quantities.

You may also adjust the two atomic masses. This supports classroom values or another reference convention. Press reset to restore standard calculator defaults.

Butane Elemental Breakdown

Element	Symbol	Atomic Mass	Atoms	Mass Contribution	Mass Percentage
Carbon	C	12.011	4	48.044 g/mol	82.66%
Hydrogen	H	1.008	10	10.080 g/mol	17.34%
Total	C₄H₁₀	—	14	58.124 g/mol	100%

Butane Reference Data

Property	Reference Value	Notes
Molecular formula	C₄H₁₀	Four carbon and ten hydrogen atoms
Molar mass	58.124 g/mol	Using C = 12.011 and H = 1.008
Total atoms per molecule	14	4 carbon plus 10 hydrogen atoms
Carbon mass percentage	82.66%	Approximate percentage by mass
Hydrogen mass percentage	17.34%	Approximate percentage by mass
Particles per mole	6.02214076 × 10²³	Avogadro constant

Example Butane Conversions

Butane Mass	Moles	Approximate Molecules
5.8124 g	0.1 mol	6.02214 × 10²²
29.062 g	0.5 mol	3.01107 × 10²³
58.124 g	1 mol	6.02214 × 10²³
116.248 g	2 mol	1.20443 × 10²⁴
581.24 g	10 mol	6.02214 × 10²⁴

Understanding Butane Molar Mass

Butane is a hydrocarbon with the molecular formula C4H10. It contains four carbon atoms and ten hydrogen atoms. Molar mass describes the mass of one mole.

Chemists express molar mass using grams per mole. This value links microscopic particles with measurable laboratory quantities. Accurate molar mass supports reliable stoichiometric calculations.

How Butane Molar Mass Is Calculated

Butane contains only carbon and hydrogen atoms. Each element contributes its atomic mass to the total. The atom count multiplies each listed atomic mass.

Carbon has an atomic mass near 12.011 units. Four carbon atoms contribute about 48.044 grams per mole. Hydrogen has an atomic mass near 1.008 units.

Ten hydrogen atoms contribute about 10.080 grams per mole. Adding both contributions gives 58.124 grams per mole. Rounded results depend on the selected precision.

Why Molar Mass Matters

Molar mass converts measured mass into chemical amount. This conversion helps determine how many moles are present. Moles can then convert into individual molecules.

One mole contains approximately 6.02214076 × 10^23 particles. This constant is known as Avogadro's number. Butane calculations use molecules because butane is molecular.

The calculator performs these conversions automatically for convenience. Enter a known quantity and choose its quantity type. The remaining related quantities appear immediately.

Mass Moles and Molecules

Mass represents the amount measured by a balance. Moles represent chemical amount rather than physical weight. Molecules represent the actual count of butane particles.

Divide mass in grams by molar mass for moles. Multiply moles by molar mass to recover mass. Multiply moles by Avogadro's number for molecules.

Divide molecules by Avogadro's number for moles. These relationships form a connected conversion system. The calculator displays each step beside the result.

Elemental Composition of Butane

Percentage composition shows each element's mass contribution. Carbon provides most of butane's molecular mass. Hydrogen contributes the smaller remaining percentage.

Carbon contributes approximately 82.66 percent by mass. Hydrogen contributes approximately 17.34 percent by mass. Together these percentages total approximately one hundred percent.

Useful Applications

Students can verify homework involving hydrocarbon stoichiometry. Teachers can demonstrate particle and mole relationships clearly. Laboratory users can estimate quantities before preparing calculations.

The tool also helps review significant figure choices. Different precision settings change displayed rounding only. They do not change the underlying chemical relationship.

Butane exists as two structural isomers with identical formulas. Both isomers therefore share the same molar mass. Their structures differ while elemental composition remains unchanged.

Reference values should match the atomic masses used. Small differences can appear between chemistry data sources. Such differences usually reflect rounding conventions.

Frequently Asked Questions

1. What is the molar mass of butane?

Butane has a molar mass near 58.124 g/mol. This uses common standard atomic masses.

2. What is the chemical formula of butane?

The molecular formula of butane is C4H10. It contains fourteen total atoms per molecule.

3. How is butane molar mass calculated?

Multiply carbon's mass by four. Multiply hydrogen's mass by ten. Then add both contributions.

4. How do I convert butane grams to moles?

Divide the butane mass by its molar mass. Use grams for the entered mass.

5. How do I convert butane moles to molecules?

Multiply moles by Avogadro's number. The calculator performs this conversion automatically.

6. Do butane isomers have different molar masses?

No. Both common butane isomers use C4H10. Therefore their molar masses match.

7. Why might another source show 58.12 g/mol?

That value uses normal rounding. Atomic mass conventions can also vary slightly.