Chemical Reactions Lab Report

The experiment is to observe a variety of chemical reactions and to identify patterns in

Equipment- 250mL beaker, 125mL Erlenmeyer flask, cardboard square, chemical scoop, metric ruler, lab countertop, rubber stoppers, safety goggles, lab apron

Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.

When the tip of the rod touched the pH paper, the color of the pH paper became blue.

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

1. Suppose that you have an unlimited supply of copper (II) sulfate to react with iron. How many moles of copper would be

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

There are now many classification systems to classify the different types of reactions. These include decomposition, polymerization, chain reactions, substitute reactions, elimination reactions, addition reactions, ionic reactions, and oxidation-reduction reactions.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

The diverse types of chemical reactions include Combination Reaction, Decomposition Reaction, Displacement Reaction and Oxidation Reaction.

The Copper Cycle is a popular experiment used to determine if an element, in this instance, copper, reverts to its elemental form after a chain of reactions. This experiment is very dangerous because of the reactions between the strong acids and bases. In this experiment I performed a series of reactions starting with copper metal and nitric acid to form copper (II) nitrate. Then I reacted copper and several other solutions such as, sodium hydroxide, sulfuric acid, ammonium hydroxide, and hydrochloric acid to form precipitates. In conclusion my percent recovery

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

Introduction: Substances can be created and can go through a chemical change. When a substance is produced this is a reaction or chemical change this is also called the product. If a substance is the reason why the experiment this is called a reactant. Whether it is a product or a reactant it depends on what happens in the chemical reaction. There is many types of chemical reactions.

There are many reaction types that can occur when compounds come together to form different types of products. In chemistry, there are eight different basic types of reactions. The eight basic reactions include: combustion, synthesis, decomposition, precipitation, single-replacement, double-replacement, acid/base, and redox reactions. These reactions are categorized into their reaction type by their differences and similarities. The first type of reaction is combustion.

Combination reactions are when two or more reactants synthesise together to form a single compound. An example of combination reactions can be seen when plants photosynthesise in order for them to nourish themselves, to do this they combine carbon dioxide from the environment and water (H2O) and convert