Purpose: The purpose of this experiment was to identify what the unknown metal was by determining what the atomic mass was. To obtain the atomic mass of the unknown metal, the number of moles of H2 gas produced from the reaction was calculated. Introduction: This lab was an application of the kinetic- molecular theory of gases. According to this theory, it stated how gaseous particles are in a constant motion where they go at random speeds as well as directions.1 According to Thomas Graham, a Scottish
the molar mass of an alcohol and the retention time of the same alcohol. The molar mass of an alcohol is a physical property defined as the mass of the given alcohol. To find the molar mass, you add all of the masses of the individual elements that make up the compound. The molar mass affects the retention time, or the rate of travel through the column, because if the alcohol being absorbed contains more mass, it will take longer for the mass to be absorbed. For example, methanol, with a mass of 32
Percent Yield Lab Questions 1) You would not be able to achieve 100% of the product because there are always ways that some of the product residue can be left over on the sides of the funnel or the sides of the beaker. 2) If you receive more than 100% yield, it means something went wrong. The precipitate could have not dried completely when the mass was taken or the filter paper mass could have been affected by the tear put in it when making the funnel. 3) It is important to know the true percent
calculations of molar masses of reactants and products within a chemical reaction. Stoichiometry tends to deal with mass-to-mass problems and often includes molar ratios, balancing equations, along with conversions between moles and grams. In order to find the percent yield, stoichiometry must be used to find the numbers needed to plug into the percent yield equation. Stoichiometry helps find the theoretical yield, which is needed to find the percent yield. For experiment six, the lab book stated the
theoretically and experimentally. The mass of magnesium oxide was calculated, when the mass of crucible, lid, and magnesium oxide was subtracted from the mass of clean, empty crucible and lid. The percent composition theoretically was found, when the mass of magnesium was divided by the mass of magnesium oxide and later was subtracted by 100 percent to get the percent composition of oxygen. Theoretically, the molar mass of magnesium must be divided by the molar mass of magnesium oxide, and also later
MOLOL VOLUME DATE OF EXPERIMENT 30/6/2015 PRACTICAL GROUP P2 LECTURER Dr. ONG SIEW TENG Title: Partial molar volume Objective: To determine the partial molal volumes of ethanol and water at a given composition by the method of intercepts. Introduction: In this experiment, we are going to use pycnometer to measure the weight of different percentage of alcohol to find out the partial molar volume of ethanol and water. Pycnometer is used because it is a glass flask that has a close-fitting ground
to express what happened (cite). For the most part, this lab used quantitative data, with the exception of noting the appearance of unknown and copper(II) sulfate. There was a linear relationship between absorbance and molarity (mol/L concentration) that was used to discover the unknown compound’s identity. The unknown was identified by comparing its absorbance to the absorbance of various dilutions of copper(II) sulfate. In lab, copper(II) sulfate was used to create a control to compare
Introduction This very experiment is aimed to determine the percent by mass in a hydrated salt (MgSO4•7H2O) in addition to getting acquainted with the equipment in a laboratory. The majority of salts occurring in nature are hydrated (water molecules bonding to the ions of the salt are the part of the structure of the compound). In some salts water molecules bond weakly to the ions and heat makes the salt to by anhydrous. During this experiment we try to identify the percentage of water contained
Purpose: The purpose of this lab was to cause a chemical reaction between magnesium and oxygen and then determine the percent composition of each substance in the final product, magnesium oxide. By doing this, the empirical formula of the product (ideally MgO) would be able to be calculated. Procedure: Clean a crucible and cover and dry it over a Bunsen burner for 3 minutes. Wait until the crucible has cooled, then measure its mass. Cut a 10 centimeter piece of magnesium ribbon into small pieces
following equation: Hydrochloric Acid + Magnesium → Magnesium Chloride + Hydrogen 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) In order to increase the rate of reaction, these following factors needs to be put in mind: The Temperature The Concentration The Mass of a substance The Pressure (For Gases) A Catalyst can also increase the Rate of Reaction. Research Question: How does changing the concentration of 5 cm3 of Hydrochloric acid influence the rate of reaction wherein the rate of the reaction will be