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Chemical Quantities by Mind Map: Chemical Quantities

1. Atomic Mass

1.1. The balanced equation for the reaction of a solid carbon and gaseous oxygen to form carbon dioxide in a gaseous way. The formula is: C(s)+O2(g) -> CO2(g).

1.2. To determine the number of oxygen molecules required, you need to know how many carbon atoms are present in a pile of carbon.

1.3. Individual atoms are too small to notice.

1.4. For counting atoms by their weight we need the information for the mass of the individual atom.

2. Molar Mass

2.1. Molar mass= mass of a substance measured in grams, moles of a substance.

3. Fórmula of compounds

3.1. A chemist determines what a compound has been formed by determine which elements are present and how much of it.

3.2. The formula represents the relative numbers of various types of atoms.

3.3. The compound contains only the elements of carbon, hydrogen and oxygen.

4. Calculating empirical formula

4.1. Rest the compound.

4.2. The mass of the oxygen present in a compound is the total mass of the product minus the mass of the nickel.

4.2.1. We first have to determine the relative masses of the various elements that are present.

5. Calculating Empirical formula for Brinary Compounds

5.1. Investigate the mass of oxygen in a simple way.

5.2. A and B represent moles of atoms in 1 mole of compounds, so we need to determine the relative number of the moles of V and O.

5.3. The values for A and B are always represented in hole numbers.

6. Calculating Empirical Formula from percent composition

6.1. The atomic masses are chlorine, oxygen and nitrogen.

6.2. The formulas are: NbH, CI and P1.

6.3. Mass percent data to get the number of moles in a formula.