Specific Heat Lab Report

1. 100 + 273 K = 373 K 150 + 273 K = 423 K 960 L x 423 K / 373 K = 1,089 L 2.

1. Gathered all required materials to designated lab bench. 2. Considered all safety precautions including the prevention of spilling water to avoid falls, handling glassware carefully to prevent shattering, avoiding long periods of working with warm water to avoid burns and avoiding the digestion/inhalation of by-products produced after the reaction (e.g. ethanol and carbon dioxide gas). 3.

The purpose of this lab is to figure out the mass percentage of copper in a penny. Furthermore, by doing this lab we will practice using a spectrophotometer and review the names of equipment such as volumetric glassware, pipets, and volumetric flasks.

Weight 30 dry pre-82 pennies which get 89.77g, using 30ml initial volume measuring the volume of 30 pennies, record the data 10.0ml. Using equation Density= Mass/Volume, get the density of the pre-82 pennies is 8.98g/ml. Then calculate the error%=0.10%, and the deviation%=1.29%.

In Lab 3.2, we burned for different chemicals and each produced a different color. The colors were different because each element, when exited, gain more energy and when the electron release that energy and jump to a more stable level/orbit, it produces a specific color that corresponds with specific wavelength that matches with each different element. Since chemicals have certain colors and wavelengths, when different kinds of chemicals are burned, you can learn what is in that chemical depending on what is produced. If a certain chemical has several blue wavelengths and only a few red wavelength, the chemical will burn blue because the blue wavelength are stronger than the red. The red wavelength will still be there but can not be seen.

1- Different elements give off different colors when heated because electrons go farther the nucleus, or to an upper energy level, and once they go back to their original orbit (energy level), they release colors because of the amount of energy released. This also happens because different elements are in different orbits and they hit different orbits as well.

In this unit we have conducted research and experiments on our chosen reactions to create the highest exothermic reaction for the The Heat-and-Eat meal pack will use a chemical reaction that involves two reactants. Reactant 1 is a solid and Reactant 2 is a liquid.

In a combustion reaction, a compound or element reacts with oxygen, releasing a large amount of energy in the form of light and heat.

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

Introduction Calorimetry is the measurement of heat absorbed or released during a chemical reaction, and in this experiment calorimetry is used to measure the amount of calories in a variety of snack foods. This is related to the saturated fat content of said snack foods. The experiment is done by setting an apparatus to burn each piece of food under a soda can full of water, this is called soda can calorimetry. A unique setup was used to determine the caloric content in each snack food. The foods used were tortilla corn chips, Lays potato chips, Cheetos Puffs, and Doritos.

The aim of the experiment will be to investigate how varying water temperatures influence the time of a chemical reaction, in this case being, a combination of Sodium Thiosulfate and Hydrochloric Acid.

In activity 17.3.2 we weighed out 150g of chilled water and 150g of pat dried ice and we put it into a styrofoam cup along with an immersion heater, and a temperature sensor. We recorded the data on LoggerPro and as the experiment is running, we continuously stirred the mixture; We ran this experiment for roughly 16 minutes; We saw that the ice was melting and once it was completely melted, the water started to get warmer and boil, we also observed steam from the water. Analyzing our data, we compared the initial mass 300g to the final mass 257.5g, there was some loss due to evaporating during the boiling process. This experiment supports the concept because we can see that when the immersion heater was melting the ice, there was a horizontal line near 0°C; When the ice was changing phase to liquid, we observed no temperature changes.

Purpose: To measure the heats of reaction for three related exothermic reactions and to verify Hess’s Law of Heat Summation.

Calorimetry is the science of measuring the change in heat absorbed or released during a chemical reaction. The change in heat can tell us if the reaction is either exothermic - it released or heat into surroundings, or endothermic - it absorbed heat from surroundings. The device used to measure calorimetry is a calorimeter. A calorimeter can range from very expensive lab ones to coffee styrofoam cups but they are all tightly sealed in order to prevent heat from escaping.

Heat transfer processes are prominent in engineering due to several applications in industry and environment. Heat transfer is central to the performance of propulsion systems, design of conventional space and water heating systems, cooling of electronic equipment, and many manufacturing processes (Campos 3).