Mole Mass Lab Report

I. Purpose: To experimentally determine the mass and the mole content of a measured sample.

II. Materials: The materials used in this experiment a 50-mL beaker, 12 samples, a balance and paper towels.

III. Procedure: As follows in Mrs. Lubin’s “Finding Moles within a Sample” Lab, found on https://docs.google.com/document/d/1m36zfJCLjGNxoswIMUya_U1HJ4agrHv2yhF6cv1JJU/edit.

IV. Data & Calculations: See attached data table.

V. Analysis:
1. Define the three identities of the mole.
The mole’s three identities include formula, molar mass or mole mass. This is defined as the mass of one mole or 6.02 * 1023 particles of that substance expressed in amu’s.
2. Explain how to determine the formula mass (mole mass) for a compound.
Molar mass is the mass (in grams) of one mole of a substance. Using the atomic mass of an element and multiplying it by the conversion factor grams per mole (g/mol), you can calculate the molar mass of that element. First, find the chemical formula for the compound. Then, calculate the relative atomic mass of each element in the compound. Next, calculate the molar mass of each element in the compound. Lastly, add the molar masses of each element in the compound.
3. Explain

Particles are labeled in many ways. One way particles are referred to be as atoms (elements). They’re identified by their properties, number or protons and neutrons and atomic number. Another way particles are referred are as molecules (covalently bonded- nonmetal to nonmetal). For example, water is a molecule because it’s composed of nonmetals. This results in elements combining together to create a molecule, with subscripts (if necessary). Lastly, particles are referred as formula units. (ionically bonded- metal to nonmetal). Labelling them include pairing a metal element to a nonmetal. This will result in elements names combining together. For example, when finding the molar mass, the label is