Ap Chemistry Butane Lab

A sample of gas is trapped in a sealed container, which has a movable lid. Moving the lid up or down will change the volume inside the container. You will use an attached manometer to measure the pressure inside the container.

To use the ideal gas law, the atmospheric pressure was adjusted for due to the lower pressure in the buret when compared to the outer atmospheric pressure. This unequalization of pressures, although corrected, may still be slightly off, thus potentially causing later calculation error when using the ideal gas law to solve for the moles of CO2.

ALKA-SELTZER GAS STOICHIOMETRY LABORATORY REPORT. INTRODUCTION The objective of this experiment was to analyze the stoichiometry, or “the determination of the proportions in which elements or compounds react with one another”, of the gas released during the chemical reaction between an Alka-Seltzer tablet and water (Britannica n.d.). This was done first by measuring the mass of the water and Alka-Seltzer tablet separately—the reactants, the environmental factors—atmosphere and temperature, and then measuring the mass of the gassy water—the products. In accordance with this experiment, many scientific concepts and topics were in play such as the Law of Conservation of Mass, stoichiometry, chemical reactions, gas laws, and the Ideal Gas Law.

The purpose of this lab was to determine the effect of temperature on the volume of gas when the pressure is consistent and to verify Charles’ Law. The data from the experiment reveals that as temperature increases, so does volume. This also indicates that as temperature decreases, the volume decreases as well.

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:

Please Note: This lab involves a lot of waiting for the gas collection. Make sure you allot yourself the full three hours to perform the experiments.

The pressure of a gas sample increases for a decrease in volume and decreases for an increase in volume.

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

Experiments 2-1 and 2-2 study the production of hydrogen gas by different chemical reactions. By using a hydrogen gas collection apparatus and the principles of chemistry, we were able to evaluate the data and reach our goal. Experiment 2-1 uses zinc, magnesium and aluminum and how much hydrogen gas they produce to predict the volume of hydrogen gas produced for different masses of each metal. In this experiment we see that each metal has an increasing amount of hydrogen gas as mass goes up, however each metal had different amount of hydrogen gas for the same mass. Zinc produced the least amount of hydrogen gas, then increasing with magnesium, and aluminum produced the highest amount. The

2. Note that the balloon in the chamber is filled with 0.300 moles of an

8. In order confidently determine what substance my “G9R” was I would have to do over the boiling point experiment a couple of more times. I would turn the gas off and take the Bunsen burner away from the apparatus when the stream of bubbles started coming out from the mouth of the capillary tube. This would allow me to correctly determine when the atmospheric pressure was equal to the vapour pressure.

The hydrochloric acid is put into a calorimeter and then the zinc is added after. The lid is closed after the zinc is added and a thermometer is inserted through the lid in order to check the temperature as the reaction takes place . The temperature is measured until the reaction has completed and the highest temperature is used as the final temperature. ∆T is then found by the equation ∆T=Tfinal-Tinitial. Then according using the equation ∆H=mc ∆T+PV. In this lab the pressure remains constant while the volume is changing. In order to calculate the volume the same reaction with the same amount of zinc and hydrochloric acid is used. However, instead of a calorimeter, an erhlenmeyer flask with a balloon put over the top is used. The hydrochloric acid is placed into a flask, the zinc is placed inside the balloon and then sealed over the flask. By dropping the zinc into the flask the reaction occurs. This allows the H₂ gas to be captured in the balloon. The circumference of the balloon is then found. The circumference can then be applied to the equation C=2πr and the radius is determined. Using the radius of the balloon, in the equation V=(4/3)πr³ the volume taken up by the hydrogen gas can be found. The pressure is the pressure of the air which is measured with a barometer. ∆H can be found by multiplying the mass of hydrochloric acid, the specific heat of HCl, and ∆T of the hydrochloric

In the fourth stage of this experiment, the density of a gas was determined. A 250ml flask was weighed with an empty rubber balloon and the mass was recorded.

The purpose of this lab was to test the law of conservation of mass by comparing the total mass of the reactants in a chemical reaction with the total mass of the product.

ABSTRACT: The aim of this experiment was calculating the values of viscosity and collision diameter for nitrogen gas, argon gas, and dry air. This objective was carried out by filling a glass bulb to a pressure of about 700 Torr with the desired gas and letting it evacuate the bulb through a capillary over a ten minute period. The pressure was recorded every five seconds. The inverse pressure was graphed against time, and a linear regression along with a least squares were performed. The slope of the line of best fit was used to calculate the capillary radius, which was then used to calculate the viscosities of the gases, which were used to calculate the collision diameters. The experimental values were compared to the literature values by percent difference, and it was found that this technique is not effective. Percent errors ranged from 0% to 30%. To make the values more accurate, the assumptions made in calculations need to be the same for all values. To take the experiment further it could be performed at other pressures, temperatures, and on other gases. Understanding properties like collision diameter and viscosity of gases are important in fields such as gas phase reaction dynamics.