Question

conclusion for chemical formula​

Answer 1

Explanation:

You need this equipment: analytical balance, Bunsen burner, 50-mL graduated cylinder, wire gauze, crucible, crucible cover, glass beads, 250-mL beaker, evaporating dish, ring stand, iron ring, stirring rod, clay triangle, crucible tongs, beaker tongs

You need these materials: granular zinc, powdered sulfur, copper wire, 6 M HCl, water

Chemical formulas are used to indicate how new compounds are formed by chemical reactions. These formulas are composed of chemical symbols. One or two letters (with the first letter capitalized) symbolize a chemical element.

Many elements are found in nature in molecular form. Two or more of the same type of atom (e.g. two oxygen atoms) are tightly bound together. The molecule behaves in many ways as a single distinct unit. A diatomic oxygen molecule would be represented by the chemical formula O2. The subscript in the formula represents the two oxygen atoms present in each oxygen molecule.

Chemical formulas that indicate the actual numbers and types of atoms in a molecule are called molecular formulas, whereas chemical formulas that indicate only the relative numbers of atoms of a type in a molecule are called empirical formulas. The subscripts in an empirical formula are always the smallest whole number ratios.

Some other important terms for this experiment are atomic mass, atomic weight, formula weight, molecular weight, and mole. Atomic mass defines the masses of individual atoms. Atomic mass units are used instead of grams. One atomic mass unit is 1.66054×10-24 grams. Atomic weight is the average atomic mass of each element. The formula weight of a substance is the sum of the atomic weights of all atoms in its chemical formula. If the chemical formula of a substance is its molecular formula, then the formula weight is also called the molecular weight. Ionic substances have only formula weights. A mole represents 6.02×1023 atoms. The mass of 1 mole (abbreviated mol) of a substance is called its molar mass. The molar mass of any substance is numerically equal to its formula weight.