Potassium Chlorate Lab

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

A mixture, unlike a compound, can be separated by physical means. There are multiple ways in which a mixture can be separated; furthermore, the ways it can be separated is based on what the mixture is made up of.

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:

What is the percentage yield of the reaction of iron and copper chloride when steel wool and copper chloride dehydrate are used as reactions?

Day 1. Michael was coming home for vacation from college. When he got home he found out that

Substances A and B have an appearance of a white solid like. Substances A and B were put into a test tube and on the Bunsen burner. As a result, B melted faster than A. A was slow to melt. The reason why B melted faster than A is because it has a lower boiling point than substance A which made it melt faster. It also shows that A needs more energy than B to be broken down.

3.6.1. BAP (Benzyl amino purine) stock solution (2mg/ml): 20mg of BAP being weighed and dissolved completely in 1N NaOH to a final total volume of 10 ml with autoclaved double distilled water to obtain a stock concentration of 2mg/ml was prepared and stored in clean autoclaved vials at -4°C.

1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow

5. Zoom Out by clicking on the green arrow next to the Save button. Click on the Stockroom and then on the Clipboard and select Balloon Experiment N2. Again, set the temperature, pressure, and moles to 298 K, 1.00 atm, and 0.300 moles, respectively. You may have to click on the Units button to change some of the variables to the correct units. Repeat the experiment with this gas labeling the data link ‘Real Gas N2.’

a) Tap and drag over the area of the graph where the resting heart rate is displayed to select the data.

In experiment 3.11, we found out whether or not a larger amount of a liquid would get hotter when it boils. To answer this, we heated a specific amount of unknown liquid and recorded the temperature every fifteen seconds. In our scatter plot, we were able to find the boiling point of our liquid. We know that the slope of our graphs is when the liquid molecules were moving around and heating up. The plateau of our graph points is where the liquid started to evaporate and boil. This is were we found our boiling point at. Shantel and I decided that our boiling point was about 98º Celsius. If you had another slope in your graph, that was when you were simply heating the leftover gas. The histogram showed us that there were about equal amounts of data in the higher temperature (about 95º Celsius) bins for both 20mL of liquid and 10mL of liquid. Also, in the lower temperature bins (75º to 80º Celsius) there was about equal amount of data for 20mL of liquid and 10mL of liquid. There was 7 pieces of data for 10mL of liquid in the lower bins, and 6 pieces of data for 20mL of liquid. If a larger amount of liquid did have a higher boiling point, the clusters would be organized by volumes or amount. For example, all of the 20mL pieces of data would be in the higher temperature bins, and all of the 10mL pieces of data would be in the lower temperature bins or flipped. Rather, the bins were clustered by identity. The boiling point is a characteristic property.

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

A hydrate is an ionic compound that has a definite amount of water as a part of its structure that it absorbs from its environment and includes as part of its structure.

When performing the experiment, the objective was to dehydrate the Barium Chloride and to find out the mass difference from when it was hydrated. Throughout the test, it was required to check the measurements of the crucible and cover for the original mass and to be able to see the difference between a hydrated and dehydrated molecule. The Barium Chloride is then placed on top of the Bunsen burner using a ring stand and carefully placing the flames under the crucible. After waiting for about 17 minutes, which would usually allow for the substance to heat up and evaporate all of the water found within it, the crucible had to cool down for about 10 minutes. After it has cooled down, the measurement would be taken again and would be less than

The difference between the two masses indicates the amount of oxygen that was released when the compound was heated. Moisture needs to be eliminated in this reaction so that the weights of oxygen and potassium chlorate can be accurate. Additionally, using the grams of oxygen, stoichiometry can be used to determine the amount of potassium chlorate that was broken down initially (Graves, 2013). Therefore, within a mixture of potassium chloride, the amount of said substance can be