 # Stoichiometry In Chemistry

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Stoichiometry is the relationship of the masses of the reactants and products in a chemical reaction. For a given mass of a substance in a reaction, the mass of any other substance in the reaction can be obtained using the coefficients of the balanced chemical equations and the molar masses of the substances involved. The amounts obtainable from a balanced chemical equation are called stoichiometric amounts (Villamar Jr., 2004).
As what was said in the introduction, the first topic that is going to be discussed is a brief background of stoichiometry and terms to remember. Based from the definition, we can derive the two parts of stoichiometry, the composition and the reaction.
Section I.
Molar Mass is the sum of the masses of the atoms that make up the formula. (i.e. Aluminum Sulfate Al2(SO4)3 has a molar mass of 342g/mol. The unit g/mol is read as grams per mole).
Table 1.1 Atomic Masses of
The compound aluminum sulfate contains 342g/mol, originally, this is 342amu but take note that the unit “amu” can be replaced with “g/mol”.
Steps in getting the molar mass of a compound:
Problem 1.1. C_12 H_22 O_11 Separate first all the elements in the compound. In this situation, Carbon, Hydrogen and Oxygen are the present elements. Know each individual element’s atomic mass (depict it from Table 1.)
Carbon – 12.01
Hydrogen – 1.01
Oxygen – 16.00 Know how many atoms of each element is present. In this instance, Carbon has 12 atoms present, Hydrogen has 22, and Oxygen has 11. Multiply the number of atoms present to the individual value of the atomic mass, and get the sum by adding all of the products.

Carbon – 12.01 x 12
Hydrogen – 1.01 x 22
Oxygen – 16.00 x 11

Write the sum with the correct unit, g/mol. In this scenario, the molar mass of C12H22O11 is 342g/mol.

Section II. Moles, Molecules, Formula Units, and

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