OBJECTIVE The objective was to determine the relationship between the reactants calcium chloride and sodium iodate their product calcium iodate. INTRODUCTION Experiment six was about the relationship between reactants and products. In this experiment the relationship of calcium chloride and sodium iodate in a reaction that produces calcium iodate. The calcium chloride and the sodium iodate undergo a precipitation reaction to produce calcium iodate. The goal is desirable for gaining understanding of limiting reagents in reactions and moles in equations. The purpose of the experiment was to determine how different amounts of calcium chloride and sodium iodate affect how much calcium iodate is produced. The chemical equation used in this reaction is: CaCl2 (aq) + 2NaIO3 (aq) → Ca(IO3)2 (s) + 2NaCl (aq) and this equation, (Concentration of …show more content…
It was observed that as increased volumes of calcium chloride was added more product was in fact produced, but it did level off. This was caused because there was not enough sodium iodate to react with all of the calcium chloride. The mole is important in stoichiometry to distinguish relationships between reactants and products. It allows you to convert between different compounds and molecules, it is also more easily identifiable. In the graph for the reaction of the experiment there should have been two clear and different slopes to represent exactly when there was an excess of sodium nitrate for the first slope and an excess of calcium chloride for the second slope. Due to the fact there is no way to have 100% yield and Graph 1 did not have two different slopes there were errors, these are some: not properly pouring the solution through the filtrate losing the precipitate under the filter paper, not rinsing the Erlenmeyer flasks completely out to filter all of the solution, and spilling any solid precipitate when removing the filter paper from the Buchner funnel or after drying when taking the
Question3: Experiment 3 The unknown acid sample was 1 • Monoprotic Acid Trails Initial NaOH solution (mL) final NaOH solution (mL) The volume of NaOH to titrate the acid (mL) Amount of Unknown Acid sample 1 (g) The moles of the Unknown Acid (mol) Molar mass of the Unknown Acid (g/mol) A 3.38 28.31 24.93 0.150 0.0026 57.69 B 0.18 29.32 29.14 0.175 0.0029
In order to find the amount of a product made during a double displacement reaction, the product has to be separated from the solution. From this number of moles of precipitate can be calculated. From there the number of moles of reactants can be calculated using the mole ratios of the particular reaction that occurred. As seen in Table 5 it is shown that by finding out the number of moles of the unknown, the molar mass of the unknown can be calculated. From the found mass of the unknown compound, the mound of the original ion can be found.
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.
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.
The test tube was quickly inverted once or twice and then poured into the cuvette and placed into the calorimeter. The absorbency readings were recorded every fifteen seconds for about five minutes, or until the reaction was complete. The same steps were followed for each of the test tubes. We then calculated the initial reaction velocity for each of the different pHs using the following equation (absorbency as y and time as
Limiting reagents can be easily determined on paper with stoichiometry, however, observing how it actually works is essential. This lab is focused on putting stoichiometry to use by determining and observing the limiting reagent in the given, balanced reaction. In the field of chemistry, many want to produce a product by reacting to reactants that will create a certain amount of a product. In order to complete this, a chemist requires a balanced equation that states the exact amounts of reactants required to produce an exact amount of a product.
The topic of this lab experiment is the relationship between percent yields and limiting reagents, and how it relates to copper (II) sulfate and aluminum foil. The objective was to determine the limiting reagent in a reaction and calculate the percent yield. To understand this, fundamental concepts of percent yields and limiting reagents are essential. A percent yield is defined as the ratio of the actual yield, to the theoretical yield in a reaction, expressed as a percent (Haberer, Salciccioli, & Sanader, 2011). This is useful as several impurities in this reaction possibly contributed to the percent yield.
The purpose of this lab is to identify the seven numbered solutions through chemical reactions. It was done by mixing the numbered solutions of known names but unknown number of distribution with each other and analyzing the chemical reactions. Research shows that NiCl2 is the green liquid. NiCl2 will not react with anything except with AgNO3 and Na2CO3, so the first step will be mixing all solutions with NiCl2 until those two chemicals are found. Na2CO3 will create bubbles (CO2) while AgNO3 does not when mixed with the other chemicals.
The topic that the scientist has researched is the reaction rate of different particle sizes. In the experiment, the scientist will discover how the particle size of Alka Seltzer affects the rate of chemical reaction with water. The independent variable in the experiment is the particle size of the Alka Seltzer, while the dependent variable is the rate of reaction, or the volume of Carbon dioxide. The volume of carbon dioxide will be measured in ml. Also, a few of the constants in the experiment will be the amount of water, and amount of tablets.
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
The limiting reagent in this lab was iron. Iron was the obvious limiting reactant because the 4.00 grams of iron was used to determine that 11.43 grams of copper sulfate would be necessary in the equation. Also, an extra 25% of copper sulfate was added to make sure there was enough copper sulfate in the reaction since it was the excess in the reaction. The theoretical yield of the reaction was 4.551 grams of copper. The theoretical yield is an amount predicted by stoichiometry and assumes that the limiting react is used completely; the yield was determined through stoichiometry by converting the amount of iron into the amount of copper in the reaction.
Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
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.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.