Molecular weight of panacetin. Convert grams Phenacetin to moles 2022-11-16
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The molecular weight of panacetin, also known as acetaminophen, is 151.16 g/mol. Panacetin is a widely used pain reliever and fever reducer that is commonly found in over-the-counter medications such as Tylenol. It is also used in prescription medications for the treatment of various forms of pain, including toothaches, muscle aches, and arthritis.
Panacetin belongs to a class of drugs known as non-opioid analgesics, which means that it does not have the potential for abuse and addiction like opioid drugs do. It works by inhibiting the production of prostaglandins, which are chemicals that cause inflammation and pain in the body.
Despite its widespread use, panacetin can have some negative side effects if taken in large amounts or for long periods of time. It can cause liver damage and should not be taken in combination with alcohol. It is important to follow the recommended dosage instructions on the medication label and to talk to a doctor or pharmacist before taking panacetin if you have liver or kidney problems or if you are pregnant or breastfeeding.
Overall, panacetin is a useful and effective pain reliever and fever reducer, but it is important to use it safely and appropriately to avoid any negative side effects.
Seperating the Components of Panacetin
The aqueous layer reacts with hydrochloric acid, the unknown component can then be isolated by evaporating the solvent from the dichloromethane solution. The purpose of this experiment is to extract the components of Panacetin. To determine the percentage recovery and melting point of the recovered benzoic acid and p-dichlorobenzene. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance. We ended up putting 129 mL of water in order to dissolve the crystals to begin the purification process. .
Crystals began to form almost immediately, even before the mixture was put into the ice bath. Also, the recovered aspirin from the first part of the experiment was recrystallized and compared to that of the isolated aspirin. Although this information is reported, the true composition of Panacetin is questionable. Data and Results: o Physical description for substance s isolated o Weight of initial panacetin sample. Acetanilide and phenacetin are not converted into salts by sodium bicarbonate. Post-Lab Questions a Isopropanol is completely miscible in water; as a result it would be impossible to perform a liquid-liquid extraction with isopropanol and water since there would not be separate layers to extract.
For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass. Introduction Acid-base extraction is a process which purifying the acids and bases from mixtures based on their chemical properties. Conclusion: In this experiment the method of liquid-liquid extraction was utilized. An esterification reaction is when an acid is converted into an ester by combining with an alcohol and removing a water molecule. When hydrochloric acid was added to sodium acetylsalicylate the solution bubbled, sizzled, and gave off heat. This whole experiment is based on purifying and then finding the melting point of the unknown compound.
When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom or group of atoms in the formula by the formula weight and multiplying by 100. These relative weights computed from the chemical equation are sometimes called equation weights. The purpose of this procedure is to isolate acetylsalicylic acid from its accompanied acid catalyst, unreacted salicylic acid, acetic anhydride, and other impurities. The reaction caused fizzing and gas. We then proceed to separate the aspirin. Discuss extraction theory and explain the general operation of the equipment? This is how to calculate molar mass average molecular weight , which is based on isotropically weighted averages.
U.S. Pharmacopeia Phenacetin Melting Point Standard, (Approximately 135
The purpose of this experiment was to determine the unknown component of panacetin. The unknown component is suspected to be a chemical relative of acetaminophen, either acetanilide or phenacetin. The aspirator was left running until the aspirin was dried and the filter paper containing aspirin was weighed as 0. Did you mean to find the molecular weight of one of these similar formulas? In order to obtain a pure compound from Panacetin, the desired compound had to be separated from the other components to by taking advantage of differences in physical and chemical properties. We then cooled the mixture to room temperature swirling the flask occasionally in an ice bath. To do this a chemist can also asses the differences between acidic and basic substances when they are added to water soluble mixtures.
Theory: Panacetin is an analgesic pain reducing and antipyretic fever reducing drug that is sold in drug stores. If successful, the percentages will be identical and the unknown component will be acetaminophen. In order to keep the body healthy, people must consume water. We collected the aspirin by vacuum filtration and washed the aspirin on the filter with cold distilled water. Calculations: Show sample calculations of the percent recoveries of sucrose, aspirin and your unknown and Rf calculations.
Explain in detail how you determined it, comparing the data you obtained with known values. Melting point range of recrystallized unknown compound. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. Order custom essay Seperating the Components of Panacetin with free plagiarism report Sucrose also ended up on the outside rim of the filter paper. We know the substance has to be Phenacetin or Acetanilide. The final product of one component, aspirin was. Pure H2O is recommeneded to conduct more precise measurement.
Next a fluted filter paper was pre-weighed. Second, we were to extract caffeine from tea. Extract the unknown solid component of panacetin, which was weighed to be 0. Water and Kerosene are opposite extremes of one another. A stirring rod was then used to stir the mixture until fizzing stopped. The release of carbon dioxide made a hissing sound. The contents of the flask were then filtered by gravity into a second dry flask using pre-weighed, fluted filter paper and a small Büchner funnel.
This mixture was then used extract the sucrose via gravity filtration. This is how to calculate molar mass average molecular weight , which is based on isotropically weighted averages. By clicking Submit, you acknowledge that you may be contacted by Fisher Scientific in regards to the feedback you have provided in this form. Technique: Show the use of separatory funnel and evaporation of solvent setup Reaction s : Include the main reaction for the experiment and isolation scheme Physical Data: List the molecular weight, melting point, boiling point, density, solubility, and hazards of all pertinent chemicals used in the experiment. Next was the isolation of the unknown analgesic.
One possible reason why the % recovery is lower than 100 % is that some of the Panacetin could have been lost during the processes of filtration and purification. Results: When we were mixing the filtration and letting it vent periodically, we lost some of it. Two layers formed, the top layer was the unknown and it was denser than the aqueous layer that was underneath it. Excercises: Lab 2 questions 1,3,5 Lab 3:1 and 2 Additional Question: Where in the separation procedure could you lose one or more of the Panacetin components? After stirring the solution thoroughly, some solid is formed solid sucrose and liquid. Such as; different boiling points, melting points and their solubility properties. Dichloromate reacts with Panacetin to produce the sucrose as an insoluble solid. After the pH reaces2, you have aspirin; which proves that as long as you follow the directions in this lab, you will have indeed separated the aspirin from the panacetin.
