Percentage of Oxygen in Potassium Chlorate, Lab Reports of Chemistry

Download Percentage of Oxygen in Potassium Chlorate and more Lab Reports Chemistry in PDF only on Docsity! Los Angeles City College Chemistry 60 EXPERIMENT 5: PERCENTAGE OF OXYGEN IN KClO3 Introduction: In this experiment you will determine the percentage of oxygen in potassium chlorate. You will calculate the theoretical value from the chemical formula and compare your experimental value to the theoretical value. Background: When potassium chlorate (KClO3) is heated, it undergoes chemical decomposition. Oxygen gas (O2) is given off and potassium chloride (KCl) remains as the residue. The equation for the decomposition of potassium chlorate is: 2 KClO3 (s) 2 KCl (s) + 3O2 (g) Other metal chlorates behave similarly when heated; forming oxygen gas and the corresponding metal chloride. The reaction may be speeded by adding some MnO2 catalyst. Metal chlorate Metal chloride + oxygen In this experiment a weighed quantity of potassium chlorate is heated. The oxygen formed in the reaction is driven off and the mass of the residue (KCl) is measured. These two quantities, the mass of the original sample of potassium chlorate and the mass of the KCl, allow us to determine the amount of oxygen in the original sample. If a catalyst is used, it will remain unaffected and its weight can be subtracted. The experimental percentage of oxygen in the sample of KClO3 is calculated by using this equation. Experimental % oxygen = Mass of oxygen lost x 100 Mass of KClO3 The theoretical value of the % oxygen in potassium chlorate is calculated from the formula KClO3 with a molar mass = 122.6 g/mol. Frequently it is interesting – and instructive - to determine the percent error of an experimental determination. The theoretical percentage of oxygen is used as the accepted value when we calculate the percent error according to this formulation. Percentage Error = | experimental value – accepted value | x 100 accepted value The numerator of this equation can be positive or negative – meaning the experimental value is high or low. In this procedure, you will be asked to heat the crucible a second time to ensure that the decomposition is complete. That means that after the first heating and cooling and weighing, the process is repeated. If the sample lost more than 0.02 g between 1st and 2nd weighings that may mean that the sample lost some more oxygen. The process of heating and cooling and weighing must be repeated until there is negligible change in mass (±0.02 g) between consecutive heatings. This is called “heating to constant weight”. Materials Needed Equipment Chemicals Iron ring, clay triangle, Crucible tongs crucible & cover or Pyrex test tube Cooling pad Potassium Chlorate, KClO3 Manganese dioxide (optional catalyst) Los Angeles City College Chemistry 60 Procedure In this experiment you may use either a crucible with cover or a Pyrex test tube. Before starting, ask your instructor as to which method you will be doing. Crucible Method: Weigh a clean dry crucible and cover. Optional, add 0.50 g MnO2 catalyst. Next, obtain a sample of potassium chlorate, KClO3, as directed by your instructor. Place about 1.5 g of KClO3 in the weighed crucible, and reweigh. Remember to use the same balance for all weighings of the same sample. Mix the catalyst well if using the MnO2. Place the crucible with KClO3 on a clay triangle and set the cover slightly ajar, see figure 1. Very gently heat the crucible containing the powders for about 8 minutes, then heat strongly for 10 minutes. Be sure the inner-blue cone of the flame is just below the crucible bottom while you are heating strongly, and that the crucible bottom and/or clay triangle are heated to redness. Allow the crucible to cool to room temperature, which takes at least 10 minutes, and then weigh the crucible and residue. Record your data in your lab notebook. Heat strongly for a second time for about 5 minutes, then cool and weigh. If the weighings after the first and the second heatings are not the same, i.e. they differ by more than 0.02 g; repeat the process of heating and cooling and weighing as needed, until 2 successive weights agree (within +/- 0.02 g). Calculate the experimental percentage of oxygen in KClO3 based on the final weight of container’s contents. Figure 1: Crucible set-up. Pyrex Test tube Method: Weigh a clean dry Pyrex test tube and beaker. Place 0.5 to 0.8 g of manganese dioxide, MnO2, into a large-size (Pyrex) test tube. (Do not use a small test tube since they are more inclined to "shoot" their contents). Measure the mass of the entire container on an analytical or centigram balance. Record the mass in the space provided on the report sheet. Add about 1.0 to 1.5 g of potassium chlorate, KClO3, to the test tube. Record the mass of the container and its contents. Mix the contents of the test tube until they have a somewhat uniform gray appearance. (Be careful not to lose any of the contents.) Carefully heat the test tube and its contents, see fig 2 below. Heat gently at first, increasing the intensity after the mixture seems to "boil," as it sometimes appears to do when bubbles of oxygen are being released. Continue heating for about five minutes, and then cool and weigh. Repeat the process in 5- minute heating cycles until constant mass is reached. Set the container and its contents aside while you complete your calculations. Do not discard the residue until your calculations are finished and satisfactory; if they are not satisfactory, it is possible that you may be able to salvage your work if the material is still on hand.