An Ice Calorimeter Determination of Reaction Enthalpy

After each of the solids were completely dry, each was placed into a MelTemp device. The temperature at which each solid began to melt and completed melting was recorded.

reaction has taken place, for example a gad is given off or a solid is

This reaction is exothermic, as heat is given out. This is because the amount reactant energy is more than the product energy the difference between this is ΔH, therefore some energy has been given out in the form of

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

3. The volume of a fixed mass of a liquid sample increases as the temperature rises from 20 to

In the third stage of this experiment, the density of a liquid was determined and compared to known standards. A 100ml beaker was filled to about half-full with room-temperature distilled water. The temperature of the water in ◦C was recorded in order to compare to known standards later. A 50ml beaker was then weighed on a scale in order to determine mass and recorded. A sample of the distilled water with an exact volume of 10ml was then placed in the 50ml beaker using a volumetric pipette. The 50ml beaker with the 10ml of water was then weighed again and the initial mass of the beaker was subtracted from this mass to obtain the mass of the 10ml of water. With the volume and the mass of the water now known, density was calculated using d = m/V and recorded in g/ml. This process was then repeated to check for precision and compared to standard values to check for accuracy. Standard values were obtained from CRC Handbook, 88th Ed.

Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring

The volume of a small test tube and a thin-stemmed pipet were determined in this section of the lab. Water was poured into a small test tube until the water reached the very top edge of the test tube. The test tube was then emptied into a plastic 25 mL graduated cylinder and volume was measured and recorded into data table 3. A think-stemmed pipet was completely filled with water. Drops were carefully counted and emptied into the empty plastic 25 mL graduated cylinder until the water level reached 1 mL. The number of drops in 1 mL was recorded into data table 3. The thin-stemmed pipet had a total volume of 4 mL and that was also recorded into data table 3.

Chemical reactions make new things by rearranging other things. In a chemical reaction, the main change that occurs relates to the way atoms are bonded to each other, in order to change those connections, bonds must be broken and new bonds be formed.

The experiment was a great way to learn how it is very hard to be 100 % error free while doing this kind of experiment. The whole class have an average of 60 or above percent error at the end of this lab. The energy was lost while heating the Mg, and Mgo in side the cubicle. Our cubicle wasn’t fully closed. There for there was a high chance of energy lost in the heat form overall and that influence the error percentage to go higher than expected. if the energy system wasn’t fully controlled there are always going to be an energy lost. The lowest error we encounter in this experiment was a a decomposition of CaCl2 salt. At the end of the experiment we got an enthalpy of – 72.3 KJ/Mole and 12% experimental error. The 12 % experimental error was by far the

an ice berg has more heat then a match because the iceberg is much larger therefore it has the capacity to hold more heat. Thermal energy is an example of kinetic energy, as it is due to the motion of particles, with motion being the key. Thermal energy results in an object or a system having a temperature that can be measured.Thermal energy can be transferred from one object or system to another in the form of heat. Describe heat transfer from hot to cold (maybe the iceberg is melting, describe change in state and particle motion).​

The literature value for the enthalpy change of the last reaction which was provided by our teacher is -97 kJ mol-1. Agreeing this value, our result can be considered accurate.

In order to obtain the true volume of volumetric glassware holds, this formula will be used.

Introduction: Every chemical change is accompanied by a change in energy usually in the form of heat. If heat is evolved, the reaction is exothermic, and if heat is absorbed, the reaction is endothermic. The energy change of a reaction that occurs at constant pressure is called the heat of reaction or the enthalpy of reaction (ΔHr). This quantity of heat is measured experimentally by allowing the reaction to occur in a calorimeter. In this experiment you will determine the heat of neutralization when an acid and a base react to form 1 mole of water. In a perfect calorimeter, heat is exchanged only between the reaction and the calorimeters water. Technically, some heat may may be absorbed the calorimeter. All calorimeters exchange some heat with its environment. This amount of heat is called the calorimeters heat capacity (the amount of of heat required to raise its temperature 1∘Celsius). We are going to “pretend” that our calorimeter is the perfect calorimeter.

In radiation heat can be transferred through empty breathing space with the help of thermal radiation.