Unknown Metals Using Calorimetry

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

Are pennies better clean or dirty? Clean, of course. Clean pennies are probably used more than dirty pennies, but maybe just clean all the dirty pennies with the products: orange juice, coca cola, and taco sauce and see which one cleans the pennies the best, so then just use those. If any of these products cleans pennies, then coca cola will clean the pennies the best. For independent variable it was the products and the dependent variable is the clean pennies. The control group is the coca cola and the experimental group is orange juice, coca cola, and the taco sauce. For this experiment there was only a few steps to do in order to have clean pennies. After all the materials are ready then pour the products into cups and put at least two pennies in each product. Once the products are in the cups then set timer for 30 minutes and repeat this step for three trials. Collect the weight of the pennies after 30 minutes each time and write it down to see which of the products took off most of the dirt on the penny. Collect all the other data that is needed. This is just one way that cleans pennies but

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.

For q, you found how much heat was gained by the water so you know that same amount of heat was lost by the metal. Therefore, qmetal = -qwater. The mass of the sample was recorded from the baggie. The temperature change

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%.

Use approximately 2 feet of aluminum foil to wrap around the burner stand and beaker to minimize heat loss.

To prepare a quantitative solution, you need to know the weight of the substance and the quantity of the solution. For example, you have 40 grams of NaOH (Sodium Oxide) in 1000mL of water. The amount of water and weight of the substance makes a Mole. one mole is equal to 1000mL of water and 40 grams of NaOH and varies by the amount of water you have but the weight of the substance must also change. To make a correct solution, you need to know the atomic mass of the substance and how much water you have in mL or L. If there are multiple elements, you need to add the combined weight of all elements (EX. NaOH= 23+16+1+40 grams.) and then divide the weight by the mass. To make a solution, you should use a beaker or flask that can measure at least

In the lab Which Is Your Metal, we attempted to identify an unknown metal by determining its specific heat capacity. We began by choosing a sample of metal, finding its mass, and describing it. We found the temperature of our boiling water. Then, we calculated the volume and temperature of the water in our calorimeter before and after the experiment. Through these calculations, we determined that the heat transferred to the calorimeter water from the hot metal was 595.65J (6.0x10²J with proper significant figures). After finding the heat transferred, we were able to calculate the specific heat capacity and match it to the correct metal. Our specific heat capacity came to 0.26J/g°C, which was closest to the

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.

Throughout the documentary, Lourdes fights to clean up the 6,000 tons of lead slag at the abandoned factory, Metales y Derivados (De La Torre & Funari, 2006, 27:02). When the factory was shut down, toxic chemicals “like sulfuric acid, cadmium, plastic, and lead” (De La Torre & Funari, 2006, 27:52) were left exposed to the elements and the surrounding community. To clean Metales y Derivados, it would take millions of dollars—money that the promotoras and Mexican government does not have (De La Torre & Funari, 2006, 29:30). Lourdes’s effort does pay off to some extent: once international media picked up the story, the Mexican government and the US Environmental Protection Agency provided her environmental justice group with US$65,000 to begin

LEARNING OBJECTIVES The learning objectives of this experiment are to. . . ! ! determine changes in enthalpy and entropy of the reaction of zinc with copper sulfate using two methods: electrochemistry and calorimetry. compare the enthalpy values obtained by the two methods. BACKGROUND Thermodynamics is concerned with energy changes that occur in chemical and physical process es. The enthalpy and entropy changes of a system undergoing such processes are interrelated by the change in free energy, ªG, according to the equation

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution.

Calorimetry is defined as the measurement of heat transfer and the amount of heat gained or lost due to chemical reactions, changes of state, or the formation of a solution (Calorimeter 1). The process of calorimetry is conducted inside of a calorimeter (Kieber 27). A calorimeter is an insulated system that thwarts heat exchange from the system to its surroundings (Toolbox 3). The main goal of this experiment is to use calorimetry to determine the specific heat of an unknown metal by using a coffee cup calorimeter, which is two Styrofoam cups nested together, and measuring the transferred heat when hot pieces of the unknown metal are submerged in cold water (Kieber 28).