Molar Mass Calculator

Molar Mass Formula:

\[ M = \sum (\text{Element Mass} \times \text{Subscript}) \]

Element 1 Mass:

g/mol

Element 1 Subscript:

atoms

Element 2 Mass:

g/mol

Element 2 Subscript:

atoms

Element 3 Mass:

g/mol

Element 3 Subscript:

atoms

Molar Mass (M):

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1. What is Molar Mass?

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It represents the sum of the atomic masses of all atoms in a chemical formula.

2. How Does the Calculator Work?

The calculator uses the molar mass formula:

\[ M = \sum (\text{Element Mass} \times \text{Subscript}) \]

Where:

\( M \) — Molar mass (g/mol)
\( \text{Element Mass} \) — Atomic mass of each element (g/mol)
\( \text{Subscript} \) — Number of atoms of each element in the formula

Explanation: The formula calculates the total mass by multiplying each element's atomic mass by the number of its atoms in the molecule and summing all contributions.

3. Importance of Molar Mass Calculation

Details: Molar mass is fundamental in stoichiometry for converting between mass and moles, determining empirical and molecular formulas, and calculating solution concentrations.

4. Using the Calculator

Tips: Enter atomic masses in g/mol and subscripts as whole numbers. At least one element must be provided. Additional elements are optional for complex molecules.

5. Frequently Asked Questions (FAQ)

Q1: What is the difference between atomic mass and molar mass?
A: Atomic mass is the mass of a single atom, while molar mass is the mass of one mole (6.022×10²³ atoms/molecules) of a substance.

Q2: How do I find atomic masses?
A: Atomic masses are found on the periodic table. For example, carbon is 12.01 g/mol, oxygen is 16.00 g/mol, hydrogen is 1.008 g/mol.

Q3: What is Avogadro's number?
A: Avogadro's number is 6.022×10²³, representing the number of particles in one mole of any substance.

Q4: Can I calculate molar mass for ionic compounds?
A: Yes, the same principle applies. Sum the atomic masses of all ions in the formula unit, considering their stoichiometric coefficients.

Q5: Why are atomic masses not whole numbers?
A: Atomic masses account for isotopic abundance. Most elements have multiple isotopes with different masses, so the atomic mass is a weighted average.