Calorimetry Lab Report

The Empirical Formula is a formula that shows elements in a compound. The molecular formula gives the amount of atoms that each element has in a compound. These formulas were used to calculate and find elements that were given prior to the crash. The formulas also helped our team find out which passengers had each of the possible materials on the flight.

The empirical formula for silver oxide for trial one is Ag5O4 and for trial two is Ag3O2. For trial one there is 0.451 grams of silver were produced from 0.504 grams of silver oxide. For trial two there is 0.456 grams of silver were produced from 0.500 grams of silver oxide. The difference between the mass of silver oxide and mass of silver is the mass of oxygen that vaporized into the air. There are 0.053 grams of oxygen vaporized into the air for trial one and 0.456 grams’ oxygen for trial two.

The filter paper should be left out overnight to dry out since all the water mass will turn into water vapor and separate from the CuO. Then scape the filter paper to get all the CuO off for it to react with excess amount of sulfuric acid, H2SO4 because the copper has to be the limiting reactant in order to get the total mass of the copper. (CuO (s) + H2SO4 (aq) -> CuSO4 (aq) + H2O (l)). Now add 0.1 g of zinc filings to the beaker and stir until the solution is colorless because originally the solution was blue from the Cu2+ so for the solution to be colorless that means all the copper has turned into a solid and all by itself (CuSO4 (aq) +Zn (s) -> Cu (s) + ZnSO4 (aq)). Finally, the solution must be filtered again to separate the copper from the ZnSO4 and the filter paper is left to dry again. The mass of the filter paper and the watch glass mass was taken beforehand again to later on subtract these measurements from the mass of the copper. The mass of the copper was weighed once the paper was all dried up and what was left was the

It used mass, temperature, length, volume, density, and making a dilute solution. I learned the importance as well as the difficulty of making proper measurements in a lab setting. If one measurement is off, it will throw the entire equation off. This will give either incorrect or inaccurate results.

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

The empirical formula is a similar molecular formula but in its simplified ratio. While calculating, you need to find the percent of a part of the compound from the whole compound. Then find the moles of each composition and then calculate mole to mole ratio between copper(II) sulfate and water to achieve the possible empirical formula. But for the mole to mole ratio to work, you need to know the law of definite proportions. It says that every chemical compound would have certain proportion, by mass, of its composition and that ratio cannot be changed. So for example a mole of water would always have 1 mole of Oxygen and 2 moles of

-Bubbles of gas began to produce itself around the aluminum which had appeared to let off vapor

The objective of this lab was to find the empirical formula of magnesium oxide. In order to produce magnesium oxide. In this experiment, magnesium reacted in an oxygen-rich environment while inside of a crucible. The masses before and after the oxidation were both measured. The masses that were resulted were then used to calculate the empirical formula of magnesium oxide. The simplest whole-number in the form of a ratio in which atoms join and form a compound is known as the empirical formula. By finding the percent composition of each element in the compound you are able to determine the empirical formula. When finding the empirical formula it is important to know how to find things such as the limiting reagent, percent yield along with the theoretical yield. The limiting reagent is a substance that will not let the reaction proceed because of its presence. The percent yield and the theoretical yield are both found by comparing the reaction and the experimental yield and recording those results.

100g of Metal Formula of Oxide Mass O2 Needed (g) Mass of Oxide Formed Lithium Li2O 115 215 Iron Fe2O3 43 143 Zinc ZnO 49 149 Lead PbO2 15 115 • “Describe the contribution of Gay-Lussac to the understanding of gaseous reactions and apply this to an understanding of the mole concept” Joseph Gay-Lussac's Law The law of combining volumes: "When measured at constant temperature and pressure, the volumes of gases in a chemical reaction show simple, whole number ratio's to each other." E.g. 1L Hydrogen(gas) + 1L Chlorine(gas)

from another. The density of an unknown substance can be determined by measuring it density in a lab.

6) Multiply by 2 to get a whole number. This ratio represents the number of magnesium atoms to oxygen atoms: the empirical formula.

In this lab, an empirical formula for the Magnesium oxide was investigated . The empirical formula of the first and second trials was calculated, and it was MgO. We used the average mass the MgO, then subtracted it from the mass of the crucible to find the mass of MgO in g. After we got the mass of MgO, we subtracted it from the m of mg to get the mass of O. We calculated the mass present of the O, then we found the molar mass of it. The molar mass of O was calculated by multiplying its mass by grams to 1 mol dividing by its standard atomic weight in (g). We found the molar mass of the Mg, then we divided the smallest value by each element in order to get a small whole number. The whole numbers for each element that are Mg and O lead us to

The colour of the precipitate was black and were quite small in size, so it was a bit hard to distinguish between the zinc powder present and the copper formed by the displacement reaction because copper formed should be reddish brown is colour – which is also a dark colour and thus two dark colours were hard to be distinguished.

calculate the molar mass of a given substance by summing up the atomic masses and then multiplying or dividing this sum by the coefficient of the substance in the chemical equation (BouJaoude and Barakat, 2000),

Number of moles of O / Number of moles of O = Moles of O per mol of O x 20 = Moles of O in Empirical Formula