An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
Abstract The main goal of this lab was to find the percent yield of a chemical reaction in which copper (II) chloride and sodium carbonate react to make copper (II) carbonate and sodium chloride. A solution of sodium carbonate and copper (II) chloride solutions were mixed to start the reaction. Then, a paper filter had to be used to separate the copper (II) carbonate precipitate from the rest of the mixture. The experiment determined the actual percent yield of 77.2%. Introduction:
Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.
For Station 4 , the magnesium and zinc turnings blackened when introduced to Cu(NO3)2 . Copper (II) nitrate, zinc nitrate and magnesium nitrate all changed colour when sodium carbonate was added. b)Magnesium is most reactive (#1). Zinc is second most reactive (#2). Copper is the least reactive (#3).
Using this number as well as the theoretical yield, the percentage yield was calculated and can be seen below in Figure 5. % Yield: (0.1805 g)/(0.3064 g) x 100 = 58.92% Figure 5: The calculations of the percent yield. The percentage yield was calculated to be 58.92% and this represents that a portion of the reactants were lost during the experiment due to a small spill or improper collection of the product during the purification process. Next, the spectrum of the product was obtained.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
In this experiment, the objective was to set up a voltaic cell and use it to carry out two electrolysis processes to determine the equivalent weights of zinc and copper. The procedure involved using zinc strips, copper strips, zinc wire, copper wire, a zinc plating solution, a CuSO4 solution, an ammeter, wooden blocks, alligator clamps, and beakers. However, the main findings of the experiment showed that the equivalent weights for both copper and zinc were not as expected. Copper had over 300
The purpose of this report is determine if sodium chloride is a viable option as a deicer on winter roads. To determine this, one must compare a multitude of factors. In this lab, the freezing point depression of water, enthalpy of dissolution, cost, and environmental impact will be discussed. A large factor in how effective a substance is as a deicer is it’s ability to decrease the freezing point of water. If the freezing point of water can be lowered, the outside temperature must be much colder to reach this new freezing point, resulting in less ice on the roads.
Using the Law of Definite Proportions, the mass of this product was used to determine the number of moles of copper and chlorine in the sample, which led to being able to determine the
The zinc will form a new compound with the sulfate, and the copper will stay as a metal. Balanced Chemical
Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.
Experiment Description: To begin the experiment, 2.0718g of a benzoic acid and p-dichlorobenzene mixture and 30 ml of methylene chloride was placed in a separatory funnel. The funnel was shook to dissolve the contents. After shaking, the funnel was inverted and the stopcock was opened to release the pressure. The stopcock was closed, the funnel was shook, and the pressure was released again. This was repeated until no more gas was released.
Zirconium is an interesting element with 40 protons, 40 electrons, and 51 neutrons. It is the 40th element on the periodic table and has the atomic symbol Zr. Its average atomic weight is 91.224. It is found as a bluish powder or as a grayish-white metal. Zirconium was discovered as the oxide Zirconia by Martin Klaproth in 1789.
First off, an empirical formula is the lowest whole number value of atoms within a molecule of a compound (Grossie and Underwood, 25). In contrast, a molecular formula can be the different from an empirical formula, in which it can be determined from the molecular weight of each element of a compound (Determining Empirical and Molecular Formula, 1). The empirical formula for hydrated copper sulfate is described in Equation 1, with x, y, and z as the subscripts that need to be determined (Grossie and Underwood,
In this research paper, I am going to investigate on how the concentration of Sodium Chloride (NaCl) solution affects the volume of the gases (Oxygen gas and Chlorine gas) at the anode during the electrolysis of sodium chloride solution. In my previous chemistry classes, I have learnt that concentration affects the majority of the gas produced at the anode. This made me wonder, how does the ratio of oxygen gas to chlorine gas produced at the anode vary at the electrodes. This made me formulate the research question: How does the concentration of Sodium Chloride solution affect the ratio of oxygen gas to chlorine gas produced at the anode during the electrolysis of Sodium Chloride solution? This area specifically interests me because it is still
