Molar mass

Discussion: The molar mass of unknown one at 0.2252 g is 248.29 g/mol, at 0.2252 g it is 248.29 g/mol, and at 0.2482 g, it is 91.25 g/mol. The average molar mass calculated is 205.07 g/mol. There was a jump in the molar mass value at different weight. This could have been due to the experimental errors that occurred during the lab. The graph of the solvent solution initially begins at 23.8˚C but jump down to 10.5˚C. This makes a huge impact on the results of the data because the freezing point should

Average Trail Mass of Sample (g) Beaker (g) Graduated Cylinder (g) Graduated Cylinder w/HCl (g) Mass of HCL (g) Mass of Beaker after Reaction (g) 1,2,3 0.491 g 94.51 g 47.70 g 67.47 g 19.77 g 114.44 g Flame test The flame was a crimson color so it was determined that the unknown substance is Lithium. Results Method Molar Mass of M2CO3 Gravimetric Analysis 78.125 g/mol Simple Weight 65.08 g/mol In the gravimetric analysis experiment, the Molar Mass of M2CO3was 78.125 g/mol. The percentage

three different methods. These three methods of flame test, simple weight loss calculation, and gravimetric analysis method were used to identify the properties and the molar mass of the unknown given sample. After doing the previous tests, it was discovered that the metal was Na2CO3 (sodium carbonate), and the mass of the molar mass was 37.158 g/mol, and the recovery rate was 95.58%. Introduction: Determining the unknown alkali carbonate was the primary goal of the lab. To distinguish the unknown

carbonate also went through a chemical reaction with 1 M hydrochloric acid, forming an alkali metal chloride, with liquid water, and carbon dioxide gas as products. A final flame test was done to reveal what the unknown alkali metal was. Once all molar masses were calculated, the masses were extremely varied, ranging from 37.061 grams per mol to 133.110 grams per mol. When the flame test was performed, yellow-orange colored flames appeared, revealing that the unknown alkali metal carbonate was sodium

Introduction Molar mass is a fundamental quantity of chemistry. There are multiple ways to find the molar mass of a substance experimentally; one way is to use Freezing Point Depression by using the following equation: ΔT= kf*m (Robinson, 2018). The purpose of this lab was to do just that; measure the freezing point depression of a solution when a solute is added to a solvent, and from that, determine the molar mass of an unknown substance, along with learning about the influence that solutes have

freezing point. Having a larger drop in freezing point is an advantage because it allows for the data to be more easily read. A large drop in freezing point also produces more significant figures and more significant figures means the calculated molar mass is more precise. 5. A pure solvent shows a level horizontal curve

Introduction This experiment had two objectives: 1) to determine the atomic mass of pure aluminum, and 2) to determine the masses of aluminum and zinc in an unknown aluminum alloy. To fulfill both of these objectives, both pure aluminum and the unknown alloy were reacted with HCl in order to produce a chemical and H2 gas. The reaction of aluminum and zinc with HCl are found below: 2Al(s) + 6HCl(aq) ⟶ 2AlCl3(aq) + 3H2(g) 2Zn(s) + 6HCl(aq) ⟶ 2ZnCl3(aq) + 3H2(g) Both metal samples would dissolve into

Background Information: This scientific report is about how much mass is lost in metals after being placed in 1 molar hydrochloric acid for 30 minutes. Tin, iron and zinc will be weighed and placed into test tubes which will then be filled with 1 molar hydrochloric acid. After 30 minutes the metals will be taken out and weighed again. It is expected that the more reaction that occurs, the more mass is lost. Tin is a metal and has many uses and is commonly used to coat other metals to prevent them

compounds. Chemical formulas can be found by a process called gravimetric analysis in which components of a compound are isolated, their masses are found, and the mass differences recorded. Gravimetric analysis can be helpful when finding the formula of an ionic hydrate, an ionic crystal bound to water molecules because it allows for the mass of water to be found allowing for further separation of the remaining elements in the ionic compound. When water is removed from an ionic hydrate, the ionic hydrate

particles might be extracted, thereby leading to an increase in the actual concentration of the dissolved salt. The weight of each 50ml beaker (used for weighing the mass of dissolved Potassium chloride after the evaporation of water) should be recorded. If the experimenter were to weigh the mass of one beaker and take it as a default mass, the latter may be a source of error. In order to minimize errors and to "place" the solutions in the same environment, the same volume should be extracted from