Lab Report On Calorimetry

The dependent variable in the experiment was the temperature and energy absorbed by the water.

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.

In this experiment, the results of the tested materials gave off heat and the change in the temperature was positive because when one substance was added to another the temperature increased. A calorimetric constant is required because the calorimeter that was made is different for every lab group.

The boiling point elevation constant for water that was experimentally determined in this analysis was 0.4396 °C/m, which was derived from the slope of the trend line in Figure 2. This is slightly lower than the constant provided in lecture of 0.51 °C/m. This could be due to further evaporation of water from the solutions tested via refractive index after the boiling temperature was recorded.

If there is an additional unmeasured amount of water in the Erlenmeyer flask, then this would reduce the concentration of the HCl, and therefore reduce the molarity. The volume of the amount of HCl solution added would increase, yet the concentration of the HCl would remain the same, which would ultimately result in the molarity of the HCl being lower than in reality.

In this experiment, a mixture of unknown #3 was used. That mixture had acid, base, and neutral. We added solvent to the unknown. It is important to know the density of the solvent in order to determine which is the aqueous layer and which is the organic layer. If the solvent that has more density than water, so the organic layer will be the lower layer, while if the solvent has lower density than water, the organic layer will be the upper layer. This will make an error if the determination of the layers was wrong after added the strong acid or the strong base. We added 5% HCl to the mixture in order to separate the base in the aqueous layer and form its salt. Same thing, we add 5% NaOH to the mixture in order to separate the acid and form its salt. In order to recover the base, we add 10% NaOH to the HCl extraction. The result will be salt with a base. Same thing for the acid, in order to recovered it, we added 10% HCl. The reaction will give us salt with an acid. For the neutral, we added sodium sulfate as a drying reagent in order to dry water and separate the neutral part as pure.

Purpose: To find the relationship between the mass and the volume of the four samples.

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

With the ∆P calculated from equation 3, ∆P is converted to dynes/cm2. The values that were calculated appear to be very similar to one another. The average ∆P are found to be ∆P= 4900(±200) ∆P= 4600 (±90) for both sides of the capillaries. The values are indicated in the table below.

There are many types of calorimeter that can be used to measure the amount of heat energy

This method of calorimetry is beneficial because it’s cheaper and more accessible than direct calorimetry. The direct method requires heavy and expensive machinery to measure the increased temperature of water surrounding a performing human. Although, this method is extremely accurate it is not as available to the doctors or researchers who’s patients would benefit by performing this test. For that reason, indirect calorimetric is a more practical method for the public.

Hypothesis: If the temperature of the chip rises, the temperature of the water above it will absorb some of the energy released by the endothermic reaction of the burning potato chip. Raw Data/ Results/ Observations: An increase in the mass of the potato chip resulted in an increase in temperature change, with the height of the water above the flame produced by the burning chip remaining constant. Although there was ½ gram more water in the second experiment, the

There are two possible reactions that can occur during an experiment. The first one is an endothermic reaction, which is when there is a flow of heat coming into the reaction. When this happens, it will be cool to the touch and it results in the products of the reaction having a higher

We will be using 6 different fuels to heat up 100ml of water, and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes, and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula:

Calorimetry, used in thermochemistry is, “the science associated with determining the changes in energy of a system by measuring the heat exchanged with the surroundings.” 3 Calorimetry is carried out with calorimeters, which measure heat transfer. 3 This experiment uses two types of calorimeters; a homemade, Styrofoam calorimeter, and a market brand calorimeter. This Styrofoam calorimeter is a less complex version of the market calorimeter and is used in some schools to save money. 4 Necessary features for a calorimeter include good insulation and little to no holes reducing heat loss to the surroundings.