I need help writing a purpose for a chemistry experiment. I feel I was always do
ID: 893917 • Letter: I
Question
I need help writing a purpose for a chemistry experiment. I feel I was always do a great job, but my professor always disagrees and I’m out of ideas. The professor wants us to summarize the introduction, and summarize what you will do in each section of the experiment and state how this work will support the goal of this experiment being longer than 1/2 a page. Please, please help me right a better purpose for the experiment below. Thanks.
The Ideal Gas Equation: The Determination of Gas Constant, R
Introduction:
For decomposition of the KClO3 in a KClO3 – KCl – MnO2 mixture, the mass of O2 can be determined by taking the difference between the mass of the original mixture and the mass of the residue after the decomposition. This mass is then converted to moles of O2 using the molecular weight of oxygen. The volume of the sample will be determined by water displacement in such a way that the pressure of the sample can be determined from the barometric pressure and the vapor pressure of water. The temperature of the sample will be directly measured.
Procedure:
Assemble the equipment for the apparatus shown in figure 1. With the Florence flask filled to the neck with water, the beaker one-third filled with water, and the pinch clamp open, blow into the tube which connects to the test to create a siphon between the flask and the beaker. Reverse the siphon a few times by raising and lowering the beaker. This will fill the tube connecting the flask and the beaker with water and will also remove air bubbles from the system. Adjust the siphon such that the flask is filled to the neck with water, and close the pinch clamp.
Weigh the eight inch test tube. Add approx. 1.5 grams of the KClO3 – KCl – MnO2 mixture to the test tube and weigh the test tube containing the mixture. Record each weight to three decimal places. (Also, be sure and record the sample number for the KClO3 – KCl – MnO2.)
Clamp the test tube to the ring stand, and insert the stopper as shown in figure 1. With the pinch clamp open, raise the level of the beaker such that the water level in the beaker is several inches above the water level in the flask. If a significant amount of water runs into the flask, there is an air leak in the system. If you have an air leak, it must be closed before proceeding. Equalize the pressure in the flask with atmospheric pressure by bringing the water level in the beaker to the same height as the water level in the flask. After closing the pinch clamp, empty and dry the beaker. Open the pinch clamp. A small amount of water will run into the beaker: this will not affect your results since later in this experiment, you will again equalize the pressure in the flask with atmospheric pressure. Ask your instructor to check your apparatus before proceeding.
Heat the mixture with a blue flame until the mixture first begins to melt and then solidifies again; and then heat for an additional 2 mins. (Don’t heat more than 7 mins.) Allow the system to cool for 15 mins. Equalize the pressure with atmospheric pressure, as before; then close the pinch clamp and open the system. Quickly measure the temperature of the gas in the flask; also measure the volume of water in the beaker. Record the barometric pressure reading from professor. Weigh the test tube with the residue and record the mass to three decimal places.
Explanation / Answer
The state of matter which had neither fixed shape and volume is gas. Gases exert pressure, and the molecules (or atoms) in a gas are separated by large distances and are in constant, random motion.
The gas law is combination of different laws
Boyle's law : Volume is inversely proportional to pressure
Charle's law: volume is diretly proportional to temperature
Avagadro law : volume is directly proportional to number of moles
Experiment: The experiment will give us the gas constant
Combined law: PV = nRT
In the first section we will measure the amount of mixture and then will measure the amount of mixture after the experiment that will give us the amount of oxygen.
so moles of oxygen = mass of oxygen / molecular weight of oxygen
Then we will measure the temperature.
By measureing the volume we can calcualte gas constant
Pv = nRT
R = PV / nT