Metal Name Mass of Metal Volume of water Initial temp. in calorimeter Initial temp. in beaker Final temp. of mixture Aluminum 34.720g 26.0mL 25.4°C 100.6°C 41.6°C Part II: Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of part II.
The concept is the same. The only trick is to keep track of which value is the actual amount, and which is the theoretical amount. Refer to the sample calculations for more insight. Equipment 100 or 250 mL beaker Watchglass Bunsen burner Wire gauze Iron ring NaHCO3 Unknown sample Examples Percent Yield from a Pure Sample A 0.685 g sample of Ca(HCO3)2 is decomposed by heating to form CaCO3. When the sample is cooled it
Then, after that we were to determine the density of the same copper cylinder by using the volume found by the water displacement method. Finally, we were attempting to identify three different unknown liquids by density determinations. Knowing the density of a certain material can be very vital to a scientist because density is used in many different ways in a chemistry lab. Undoubtedly the most important use of density is the ability to determine an unknown substances identity. Since every material has a unique density a scientist can simply calculate the mass and volume of an object, find the unknown object’s density and he will, without a doubt, have correctly identified the substance.
Then prepare the unknown sample by pipetting 1 ml of the unknown solution into the cuvette and mix with 1 ml of dilute ferric nitrate. Then after that you calculate the concentration for each of the solutions. Cuvette # | 25 mg/dl Standard | H2O ml | Dilute Iron III Nitrate (ml) | .039 M HNO3 (ml) | Concentration | 1 | 0 | 1 | 0 | 1 | 0 | 2 | 0.1 | 0.9 | 1 | 0 | 0.09 | 3 | 0.3 | 0.7 | 1 | 0 | 0.287 | 4 | 0.5 | 0.5 | 1 | 0 | 0.407 | 5 | 0.7 | 0.3 | 1 | 0 | 0.706 | 6 | 1 | 0 | 1 | 0 | 1.316 | When then use the calibration curve to determine the concentration of the unknown and we get .747. IV. As you can see from our data as the amount of H2O decreases and the 25mg/dl standard increases as does our concentration for the salicylic acids.
Martin Deng 19/02/2012 11 Chemistry E T13P 8.2-5.3.1 perform a first-hand investigation to compare the properties of some common elements in their elemental state with the properties of the compound(s) of these elements (eg magnesium and oxygen) Chem.p1.53 Dot. pt.Pre.Chem. p 34 T13P: Comparison of properties in elemental and compound state T13P: Comparison of properties in elemental and compound state Introduction: The idea of this practical experiment is to understand properties of common elements in their elemental state and in their compound state. The processes that are to be used in this experiment are synthesis, oxidation and combustion. It also involves the changing of elements into a compound.
Mariah Munson Lab, Week #1 BALANCE LAB Introduction <Include purpose of lab experiment> The purpose of the Balance Lab is to learn how the ILab works and also how to correctly determine the mas of a chemical. <Brief summary of topic investigating> We will lean how to read the mass off the balance, and how to find a weight of an item that is measured in a container, and how to use the centigram balance. <State major finding> I learned what the centigram balance is, it has two decimal place precision. Procedure <Include information that the reader would need to repeat your experimental procedure. Do not include any observations or results in this section?
PURPOSE/INTRODUCTION The purpose of this experiment is to produce visible emissions from heating different metal fluorides with a Bunsen burner. The hypothesis is that by warming the different metal chlorides, the different elements found in each chloride will produce a different color when placed in the flame. We will also produce a table of our findings with our information we recorded from the results gathered in this lab. In the preceding discussion, we will be testing different metal chloride reactions when a flame is introduced to them. MATERIALS * One Bunsen burner * 1 gram of Sodium Chloride * 1 gram of Potassium Chloride * 1 gram of Lithium Chloride * 1 gram of Barium Chloride * Nichrome wire (wire with a loop) * 0.4 grams of water * Protective eyewear * Lab gloves Barium is a toxic metal, be sure to wear gloves and goggles when handling this material, also if using a Bunsen burner be sure to turn of the gas.
Show ALL your work. Use the given specific heat capacity values below to calculate the percent error of the experimental specific heat capacity that you determined in Part I of the lab. Known specific heat values — Iron: 0.444 J/g°C; Zinc: 0.390 J/g°C; Copper: 0.385 J/g°C, Aluminum: 0.900 J/g°C Percent Error == | experimental - actual value | / actual value x 100 % Using the specific heat capacity value that you determined in Part II of the lab, what is the most probable identity of the unknown metal that you examined? Please explain your reasoning in complete sentences. I believe the most probable identity of the metal is Silver because it is the closest to the experimental heat value.
The purpose of the following experimentation was to use two intensive physical properties, specific heat and linear thermal expansion, to determine if a sample of an unknown metal was Zinc. Throughout the course of experimentation, data from the unknown metal was compared to values from the known metal. The ultimate goal of the experiment was to use this data to identify the unknown metal. But in order to find these values, two experiments were conducted. The first of the two experiments was based in calorimetry.
Specific Heat By: James Ott Date: January 1, 2013 PURPOSE/INTRODUCTION The purpose of this experiment is to measure the temperature of metals, and estimate the specific heat for a metal. This experiment is also an introduction to the use of a calorimeter. This is a good way of using a known amount of metal and a known temperature change. The calculation for finding specific heat of a metal is: q=s x m x Δt MATERIALS Materials required complete the lab: * Test tube * Bunsen burner * 100 g Iron (Fe) shot * Thermometer * 250 ml beaker with 150 ml Water (H2O) in beaker at room temperature * Calorimeter with 100 ml Water (H2O) at room temperature * 100 g Aluminum (Al) shot * 100 g Copper (Cu) shot METHOD * Set up one test tube * Add 100g Iron shot and thermometer * Setup a 250 ml beaker with 150 ml room temperature water * Place filled test tube in beaker * Setup a Bunsen burner * Hover beaker over Bunsen burner until thermometer reads 100˚C * While beaker is warming, set up calorimeter with 100 ml of room temperature water (20˚C) * When metal temperature reaches 100˚C, remove from beaker and pour liquid into calorimeter, close lid and read thermometer reading * Record reading * Repeat above steps for other two metals DATA Metal | Initial Temp. (˚C) | Final Temp.