Mole

pressure, and volume are all accounted for. Dalton’s law of partial pressure is another theory that was explored in this lab. It states that the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases. This law makes it possible for the partial pressure of the water vapor to be removed from the total pressure of the gases in the eudiometer tube to yield the partial pressure of hydrogen gas. Molar volume is the volume occupied by one mole of a gas, in this case, hydrogen gas. Molar volume relates to the lab as the entire purpose of this lab is to find the molar volume of hydrogen gas at STP. The ideal gas law describes a relationship between pressure (P), volume (V), the number of moles (n), temperature (T), and the universal gas constant (R) where PV = nRT. This ideal gas law is essential to the lab as it explains the relationships between the different measurements of a gas and reduces into the combined gas law. The combined gas law is a relation where the number of moles of gas is constant, thus leaving the variables of pressure, volume, and temperature. When comparing the same substance under different conditions, the combined gas law can be mathematically written as (P"1" V"1" )/T"1" = (P"2" V"2" )/T"2" . Since the conditions of the experiment were not at standard temperature and pressure, the combined gas law is required in order to calculate the corresponding volume of hydrogen gas at STP. Single displacement reactions were…

until a mustard color is obtained. Starch is then added to amplify the visual cue as explained before. The solution is then titrated to a milky pink and KSCN is added just before the endpoint. The addition of KSCN is necessary since iodine molecules have a tendency to occlude on the surface of CuI and thus, is not readily reduced by thiosulfate. SCN- can compete with this occlusion and free up the iodine so it can be reduced by thiosulfate. Finally, the solution is titrated until a sudden…

Hoff factor for a solute is equivalent to the number of particles, in moles, will break apart in the solvent. When an…

Formal Lab Report: Molar Volume of a Gas at STP Abstract: The purpose of this experiment is to find out how to experimentally determine what the volume of a mole of H₂(g) is at STP by using gas laws. The hypothesis for the experiment is that if H₂(g) is produced at RT and STP, Avogadro’s law can be used to experimentally determine the amount of H₂(g) because equal gases at the same pressure and temperature have the same amount of particles. In order to find the molar volume, hydrogen gas…

The problem of the experiment was to determine the volume of one mole of H_(2(g)) at STP. In a way, the problem is essential in understanding how one mole of an ideal gas at STP is always equivalent to 22.4 L. By determining if the volume of a mole of H_(2(g)) is 22.4 L, it supports Avogadro’s law that one mole of an ideal gas occupies 22.4 L at STP. At the same time, it indicates that a direct relationship exists between volume and the number of moles of gas as temperature and pressure stays…

wasn’t just making cool stuff and playing with rocks, it was math. We did have an earth science class in 9th grade, with Mr. Tvedten. He really loved rocks. I thought the unit was boring but his enthusiasm for the subject at least gave me motivation to pay attention during notes. In 11th grade, I had chemistry with Mrs. Hei. I loved this class because we were trusted with fire and chemicals that were potentially dangerous. How many high school classes can you say that about? This class had a lot…

M) * MM(CH3COOH) (0.5967M) * (65.05 g/mol) = 35.85 g/L 4) Percent Acid ((g/L)/(given density)) * 100 ((35.85 g/L)/(1005 g/L)) * 100 = 3.57% UNKNOWN ACID 1) Moles of NaOH ((Vf - Vi)/1000) * M Run #1: ((31.11 – 0.51)/1000) * 0.2116m = .006475 Run #2: ((31.35 – 0.38)/1000) * 0.2116m = .006553 2) Calc Moles of Acid because 1:1 ratio moles acid equals moles NaOH moles acid = Run 1: .006475 and Run #2: .006553 3) Molar Mass (grams used/moles acid) Run #1:…

experiment was actually conducted. There could be a pressure difference between the two labs and this could in turn change the values of the data. There was also a variety of data that was provided or given. For example, the diameter of the syringe plunger was given to be 0.90 inches and this could actually not be the true value of the diameter of the syringe plunger. Another example of given data is the atomic masses provided by periodic tables that was used to calculate molar mass in…

Moles 1.How is molar mass calculated and why is it useful? Molar mass is calculated by going to the periodic table finding each mass of each element in the compound then adding them all up based on how many of those elements are in the compound. 2.Define a mole in chemistry and give 3 examples equivalent units that are used in chemical calculations. Mole is considered the unit for amount in chemistry other units that are equivalent are atoms, formula units, and molecules. Gas Laws 3.How is the…

Introduction Section- The purpose of this experiment is to use reaction stoichiometry to determine the molar mass and the identity of an unknown, powdered metal, and to identify an unknown metal nitrate solution. To give a little background information on this experiment I will start by saying that a balanced chemical equation provides several important pieces of information about a chemical equation. Those important pieces include the substances consumed and formed, the physical states of the…