Coke Calorimeter Lab Report

2) Heat one to about 50˚C, and place other one in calorimeter (at around 20˚C)

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

Our task was to identify the powder in each bag containing different amounts of moles. The mole provides a standard unit of measure that can be used to compare a wide variety of substances. A mole of atoms gives you a physical representation of what a single atom. The molar mass is the total mass of an element divided by one mole in that element. The molar mass can be used as a physical property to identify unknowns by converting it to moles and seeing which one is the closest to the moles in the bag. Our guiding question to answer was: “What are the identities of the unknown compounds?”

We did our experiment using popcorn and bread. First we measured the mass of the pieces of bread and popcorn and we weighed their mass. We added 10cm of water into a test tube, measured the temperature. We heat the water with the help of the fire that caught on the food substance and we measured the temperature at the end when the food had completely burnt out. To find the energy released we used the formula, energy released = mass of water (g)*temperature rise *4.2/ mass of food sample (g)

The materials we used for this experiment were two aluminum soda cans, water, ice, a graduated cylinder, a metal saucepan, a hot plate, and a

The first trial that contained 10 mL of NaOH and 10 mL of CH3COOH produced a ΔHrxn of -13.11 kJ/m. The second trial, which contained 15 mL of NaOH and 5 mL of CH3COOH resulted in a ΔHrxn of -7.864 kJ/m. Based on the literature value of NaOH CH3COOH, -57.5 kJ/m, we were off by 44.39 kJ/m in the first trial, and 49.64 kJ/m in the second trial.

As for the part two the experiment, the class was divided into two groups and both groups were specifically assigned to determine ΔS and ΔH. In order to determine ΔS and ΔH, the calorimeter apparatus was set up first. After, the materials that were also needed was the igniter and the fuel. The lab coordinator provided the groups with those materials. The igniter was initially weighted and was determined to be 0.057g. After, the initial weight of the igniter was recorded, it was then inserted to bottom of the fuel. Then the combination of the igniter and the fuel before the combustion was weighed, which was 0.647g. The igniter

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).

My hypothesis heading into this experiment was that the closer the flame was to the aluminum can, the higher the temperature/heat would be. This concept is pretty self-explanatory because fires are very hot and so if you put any object near a flame, the object will start to heat up. Setting up/completing this lab

Following in the steps of Lavoisier and Pierre-Simon, an experiment will be conducted on the heat capacity of a Styrofoam calorimeter in comparison to a brand calorimeter. Water shall be used first because of its known specific heat and the experiment will be repeated with HCL (Hydrochloric Acid) and NaOH (Sodium Hydroxide) in hopes to calculating the specific heat of the reaction.

What will be the amount of energy contained in specific snack foods? This question will be solved by using the heat energy equation, Q=mCΔT. “Q or q” will represent the heat in joules, this will be found algebraically by filling in the rest of the heat energy equation. “m” will represent the mass in grams, this will be found by finding the mass of the water. “C” will represent specific heat in Joules/grams °Celsius, the specific heat of water will always be 4.184 J/g°C. “ΔT” will represent the change in temperature, this will be found by subtracting the final temperature of the water by the original temperature of the water. Capital Q means that heat will be added-endothermic. Lowercase q means that heat will be lost-exothermic. The law conservation of energy says that energy will not be created nor destroyed, but will be converted from one form to another. The percent error equation will be (accepted-experimental) ÷ (accepted), accepted is the Cal/g on the snack food’s package, and the experimental is the Cal/g that is calculated during the experiment. The independent variable will be the Marshmallow, CHEEZ-IT, Cheetos, and Chex-mix. The dependent variable will be the energy in either Joules/grams or Calories/gram because the amount of energy depends on the snack food. The controlled variable will be the amount of water in the calorimeter because the water will be the same amount in every trial. A bar graph will be needed to determine which snack food

Results from the experiment showed mass specific metabolic rate to increased as temperature decreased. An increased in metabolic rate is a result of an increased in respiration rate required from the mice to maintain internal body temperature at 37℃. Therefore, the hypothesis was supported because experimental data revealed respiration rate to increased as environmental temperature decreased. Experimental results can be supported by several published primary literatures that showed how environmental temperature affected an organism’s metabolic rate.

The purpose of the experiment is to determine the enthalpy of neutralization reactions by calorimetry. Calorimetry, is the science of measuring the amount of heat. All calorimetric techniques are therefore based on the measurement of heat that may be generated (exothermic process) or consumed (endothermic process). The device used for measuring the heat changes in this experiment is called calorimeter. A calorimeter is a Styrofoam cup is used as a calorimeter, because it is a container with good insulated walls to prevent heat exchange with the environment.

Use the forceps to transfer the metal sample quickly from the beaker with boiling water into the calorimeter. Cover the calorimeter with the lid and insert the thermometer.

On the first week, the first activity done was to construct a handmade calorimeter using two Styrofoam cup placing them into each other and cutting out a cardboard as a lid making sure the cardboard is big enough to cover the Styrofoam cup. After that is done puncture the lid creating two holes; one for the stirrer to stir the solution and the other for the thermometer to check the temperature of the solution, the cup was then weighed as 31.67g. After getting that done as the purpose of the experiment is to measure the change in heat; 50ml of water was measured using a graduated cylinder, poured into a 100ml beaker then placed on the heater. But before it was placed on the heater the initial temperature of the water was checked by placing the thermometer into the water coming out to be 24oC which is roughly room temperature. The water was left to heat up to 52oC, it was then transferred into the Styrofoam calorimeter to get the final temperature which was 37oC. After getting done with the wet hand part of the experiment, the enthalpy and specific heat of the calorimeters had to be calculated using the formula Q= MCDT. Where Q- heat, M- mass, C- specific heat, DT- change in temperature. These same procedure was done using the commercial calorimeter, performing three trials for each.