Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Chemistry chapter 14 gas laws
Chemistry chapter 11 on gas laws
Chemistry chapter 11 on gas laws
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Chemistry chapter 14 gas laws
Vapor is the gas that forms from the vaporization of a volatile liquid. Dumas or vapor density was the method used and is done by measuring the mass of the vaporized liquid and the volume occupied by the vapor. Ideal gas law was the equation used to solve for the molecular mass of the unknown volatile sample. The purpose of this experiment is to determine the molecular mass of a substance from measurements of the density of its vapor. For the methodology, water was heated to boiling. Cap was prepared and been weighed together with the 125-mL flask. Unknown was placed in the flask and was lowered when the water reached its boiling point. It was continuously heated until the entire sample evaporated. Flask was then removed and allowed to condense. Mass …show more content…
The gas collected will be measured under the laboratory conditions of temperature and pressure. Ideal Gas Law relates the number of moles of a particular substance in a gaseous state with its volume, temperature, and pressure (Equation 1). Hence, the Ideal Gas Law can be used to determine the molar mass of a volatile liquid from the density of the vapor. Molar mass is defined in terms of the mass in grams of a substance per mole of that substance, g/mole. Equation 2, which is derived from the Ideal gas law, will be used in solving the molar mass of the unknown substance (AP Chemistry, 2010). Equation 1: Ideal Gas Law Equation 2: Equation derived from Ideal Gas Law II. OBJECTIVES The purpose of this experiment is to: 1. Determine the molecular mass of a substance from measurements of the density of its vapor. III. MATERIALS AND METHODS Materials to be used will be 125-mL Erlenmeyer flask, 400-mL beaker, iron stand, iron ring, clamp, crucible tongs, 100-mL graduated cylinder, thermometer, aluminum foil, heating stove and burner (if possible). Reagent needed for the experiment was the unknown liquid
The purpose of this lab was to determine the density of water and an unknown liquid, along with a rectangular solid and an irregular shaped solid. In this lab, the relative density was calculated and then used to make an educated guess on the substance. Density is the relationship between the mass of a substance and the amount of space taken up. This measurement is influenced by the mass of atoms, the size, and how they are arranged. The density of the four objects was determined by using the mass (g) and volume (mL or c3). Mass is the property of matter that measures its resistance to acceleration. In addition, volume is the amount of space that a substance or object occupies. Finally, the mass (g) was divided by the volume (mL or c3) to find the final density (g/mL or c3).
This law, known as Gay-Lussac’s law, observes the relationship between the pressure and temperature of a gas. Contrary to its name, this relationship was actually discovered by French scientific instrument inventor and physicist Guillaume Amontons, and is occasionally referred to Amontons’ Law of Pressure-Temperature. While Guy-Lussac did explore the temperature-pressure relationship, Guy-Lussac’s law is usually used to refer to the law of combining volumes. Amontons stubble across this relationship when he was building an “air thermometer.” Although not many have been able identify his exact method of experimentation, later scientist developed an apparatus in which consisted of pressure gauge and a metal sphere. These two pieces were then attached and submerged in solutions of varying temperatures. From Amontons’ and Guy-Lussac’s research and experimentation, they determined that pressure and volume had direct relationship; as one increased, the other increased. The quotient of pressure and temperature was then found to equal a constant, in which just like Boyle’s law, could be used to find one of the two variables at another pressure or temperature, given one of the variables and that the other conditions remain the same. Instead of using various solutions at different temperatures like in the experiment describe above, many experiments today utilize a solution in which the temperature is increased or decrease, such as in the following
Aim: - An experiment on how a volume of nitrogen gas is affected by the pressure exerted on it.
Introduction and Background : The molar mass of a gas relates to the number of grams in one mole of that particular gas and all molar masses can be found on the periodic table of the elements. The objective of this lab is to compare the theoretical value of butane gas’s, C4H10 (g), molar mass with an experimental value where the gas from a lighter was released and measured by testing if the water displacement method, where a graduated cylinder is inverted in water and gas is released beneath it and trapped in the cylinder, is reliable for collecting data due to it being combined with water vapour as well. After the volume and mass of the gas released are measured, the number of moles can be found by subbing all known variables, including temperature
The molar mass of my unknown is 96.835 g/mol; the density is 0.8601 g/Ml; the boiling point is 68.5℃ and the molecular and empirical formulas are C_4 H_9 Cl. (Table 1) The molar mass of 2-Chlorobutane is 92.039 g/mol; the density is 0.87 g/mL; the boiling point is 69.2℃; and the empirical and molecular formulas are C_4 H_9 Cl. (ChemSpider) The properties all match up and they helped me identify my unknown. During the experiment and the later research that followed, I learned how to identify what a compound using its intrinsic properties and how isomers function in the real world. I found out that 2-Chlorobutane has an estimated amount of 6 isomers and that shape sometimes does define how a compound works. The isomers all have the same formulas, however the differently arranged bonds change the whole compound. I also learned how to measure the atmospheric pressure using a barometer in the classroom and this experiment really improved my understanding of Chemistry concepts involving mass calculations. One of the most important concepts I have learned from this research paper and my data analysis, is that good Chemistry experiments require more than 2 trials and precise procedures that can be
The goal of this lab is to apply principles of the ideal gas law to solve for n or the number of moles carbon dioxide produced, and compare the amount found using the ideal gas law to the actual amount. In order to complete this lab it's necessary to understand the apparatus below. By filling the Erlenmeyer flask completely full with water the mass of CO2 gas in the top of the flask can be determined. Since the combination of sodium bicarbonate and oxalic acid produces CO2 gas, this gas then moves from the gas generation bottle into the tube connected to the pneumatic trough. This gas then moves through the hole in the trough into the Erlenmeyer flask. The gas rises to the top and then pushes the water down and out. By measuring
The Equation Of State These three gas laws that were proposed by Boyle, Amontons and Charles can be summarised as follows: For a fixed mass of gas pV = constant if T = constant (i) p/T = constant if V = constant (ii) V/T = constant if p = constant (iii)
Thanks to Avogadro and his number, scientists can measure out equal number of molecules by weighing out an equal number of moles. For gases this can be done by using 22.4 liters at STP(1 atmosphere and 223 Kelvin, 0 deg. Celsius). Avogadro's number is most reliably determined by X-ray diffraction of crystals.
In experiment’s 2rd trail, a new calorimeter was placed onto the workbench. It was placed onto the electronic scale and weighed 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature was 21.5 C. 50 mL of 1M Hydrochloric Acid was placed into the calorimeter. 0.250 grams of magnesium was placed into the calorimeter. A chemical reaction occurred and the temperature recorded was 43.2 C. The calorimeter was placed onto the electronic scale and weighed to be 68.839 grams. Afterwards, the calorimeter was discarded. In the experiment's third trial, a new calorimeter was placed onto the workbench. It was then placed onto the electronic scale and it weighted 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature recorded was 21.5 C. 50 mL of 1M Hydrochloric Acid was placed into the calorimeter. 0.350 grams were added into the calorimeter. A chemical reaction occurred. The recorded temperature is 51.8 C. The calorimeter was placed onto the electronic scale and the total mass is 68.921 grams. All materials were
One of Boyle’s most well known discoveries is Boyle’s law. This law was named in his honor for being the first to discover it. According to the Glenn Research Center, for a given mass, at constant temperature, the pressure times the volume is a constant, meaning when the volume increases, the pressure goes down, and when the volume decreases, the pressure goes up The formula for his law is p * V = C. In the formula, p stands for pressure, V stands for volume, and C stands for a constant. When Boyle’s Law is combined with Charles’s law, it will produce the Ideal Gas Law, which states The law states that P × V = n × (R) × T, where P is pressure, V is volume, n is the
Mole relations: One mole (abbreviated mol) is equal to 6.02×10 23 molecular entities (Avogadro's number). Each element has a different molar mass depending on the weight of 6.02×10 23 of its atoms (1 mole). The total number of atoms of each element must be the same on each side of the equation to satisfy the Law of Conservation of Mass. The experiment aides in the understanding of mole-mass relationships that exist in a chemical reaction and in the interpretation of a balanced chemical equation.
Mass spectroscopy originated in 1919 by a British scientist named Francis Aston when a machine was created for the purpose for measuring the proportions and masses of the atomic species in part of a sample. A mass spectrometer is an instrument that measures the masses of individual molecules that have been converted into ions e.g molecules that have been electrically charged. A Mass Spectrum is a plot of ion intensity as a function of the ion's mass-to-charge ratios. Spectroscopy is a diverse and complex branch of science. It has many uses and is widely acknowledged as an essential part of development in the world of science.
In this experiment the relationship between volume and pressure and the relationship between temperature and volume are explored with the LabQuest pressure sensor. First, the sensor and a syringe were used to find the relationship between volume and pressure by changing the volume within the syringe while it was connected to the sensor. Next the sensor was connected into an Erlenmeyer flask which was put into boiling water that was slowly lowered to 0○ to measure the change in pressure while the temperature dropped. The first relationship is called Boyle’s Law and was originally found by Robert Boyle, who published it in 16621. This law is now used to carbonate sodas. By pressurizing soda cans, the CO2 gas inside it is forced to dissolve, and when the can is opened, the pressure is relieved, and the gas begins to
In gaseous flows, the density of gas becomes a field variable whose value depends on the temperature and local pressure.
Gases are everywhere. Although you may not be able to see them you are surrounded by gases. Gases are in soda/pop, a hot air balloon, the tire on a bicycle and they are even in the air we breathe. There are many gases in the air we breathe. Air contains a mixture of gases including nitrogen, oxygen, argon, carbon dioxide and water vapor. Nitrogen, Oxygen, and Argon make up the greatest amount of air. Nitrogen makes up about 78% of air. Oxygen comprises approximately 21% of air. Argon constitutes 0.934%. All gases have similar physical properties. The physical properties of gases include four variables. These four variables are pressure, volume, temperature and the number of moles. These four variables can be arranged in an equation, the equation being PV=nRT. This is called the ideal gas law. One of these four variables can be figured out as long as you know the other three variables. This leads people to believe that these four variables are interdependent.