How do you find the molar mass from the atomic mass?

The molar mass of a compound is found by adding up the atomic masses of all the atoms present in its chemical formula.

Understanding Atomic and Molar Mass

Atomic Mass: This is the mass of a single atom of an element, typically expressed in atomic mass units (amu). You can find the atomic mass of each element on the periodic table.
Molar Mass: This is the mass of one mole of a substance, expressed in grams per mole (g/mol). One mole is equal to 6.022 x 10²³ entities (like atoms, molecules, ions).

Based on the reference material in the provided text, calculating molar mass involves the following steps:

Identify the Chemical Formula: First, determine the chemical formula of the compound you're working with (e.g., H₂O for water).
Find Atomic Masses: Locate the atomic mass of each element from the periodic table.
- For example, as mentioned in the reference:
  - The atomic mass of hydrogen (H) is approximately 1 amu.
  - The atomic mass of oxygen (O) is approximately 16 amu.
Multiply by Subscripts: If there's more than one atom of an element in the formula (indicated by a subscript), multiply the atomic mass by that subscript.
- For example, H₂O has two hydrogen atoms, so we'd multiply the atomic mass of hydrogen by 2.
Add Atomic Masses: Add the results of step 3 together to get the molar mass.
- Continuing with the H₂O example:
  - (2 x Atomic mass of H) + (1 x Atomic mass of O) = Molar mass of H₂O
  - (2 x 1 amu) + (1 x 16 amu) = 18 amu
Convert to grams per mole: Since 1 amu = 1 g/mol, this atomic mass is also its molar mass, expressed in grams per mole.
- Therefore, the molar mass of H₂O is 18 g/mol.

Based on the video description:

Find the atomic mass of hydrogen (H) and oxygen (O) on the periodic table.
Multiply the atomic mass of hydrogen by 2, since there are two hydrogen atoms in water (H₂O).
Add the result to the atomic mass of oxygen to get the molar mass.

Using Molar Mass: Molar mass is essential for converting between mass and moles, which is a critical step in stoichiometric calculations, allowing you to quantify reactions using units like grams or moles.
Accurate Calculations: For more accurate calculations, use the atomic masses from the periodic table that are expressed to more decimal places.