The Decomposition of Potassium Chlorate Essay

with a solid oxidant that is composed of KMnO4 and CuSO4. 1.0mL of diphenylmethanol was placed into

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

2. The second source of error in the lab is when opening the lid of the crucible which allowed smoke of magnesium oxide to escape. During the lab, we removed the lid a couple of times to allow oxygen to enter the crucible so the magnesium reacts with the air to form magnesium oxide. However, the smoke could have easily escaped from the crucible because of the strong force of heat from the laboratory burner. This could have affected the lab results by decreasing the final mass when some of the product have escaped.

The first experiment is about the combustion of magnesium after which the ash is formed.

For our second procedure our first step was to gather materials of a 2 cm long magnesium strip, a bunsen burner, and crucible tongs. After we gathered materials we turned the gas to the bunsen burner on, carefully lit the burner with our striker, and adjusted the flame. We then used the crucible tongs to pick up the magnesium strip and place it in the flame, keeping it a safe distance away. Lastly, we recorded and watched our reaction.

Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction:

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.

| After ignition of magnesium light and toxic fumes are made, and white powder (2MgO or Magnesium Oxide) is left over.

Place the test tube containing cold water in a test tube clamp and hold the test tube above the burning alcohol. Observe the outside of the test tube for evidence of product formation.

To see if the concentration of hydrochloric acid will increase the rate of the reaction between magnesium ribbon and hydrochloric acid.

I predict that the reaction will begin rather quickly with the addition of the enzyme, but will slow as the H2O2 is converted to H2O and O2. I also believe that, given the amount of time the reactions are to be run for, not all of the H2O2 will react, thus leaving some to react with the KMnO4 even after the full 360 seconds.

A more detailed explanation of procedures can be found in the lab packet.1 To summarize, samples of benzoic acid and naphthalene were combusted using the Parr 1341 Calorimeter with a Parr oxygen bomb. A massed benzoic acid pellet was placed onto the center of the combustion pan and 10 cm of nickel alloy fuse wire was massed and then threaded through both electrodes on the head of the bomb so that it lay firmly against the acid pellet. 1mL of distilled water was then placed in the bottom of the bomb in order to ensure that all the water produced by the

Safety glasses: Wear safety glasses to protect eyes from substances, acids and flames that can irritate or damage the eyes.

A ring stand and ring clamp were set up with a Bunsen burner an inch below to allow for the optimal heating. The Bunsen burner was not lit at this time.

Part A.1. Sodium metal is also readily oxidized by oxygen. If the product of the reaction were dissolved in water, what would be the color of the litmus for a litmus test? Explain. What is the product?