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Lab report for calorimetry and specific heat
Experiment 25 calorimetry introduction lab report
Lab report of calorimetry
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The heat of solution is the enthalpy change associated with the process of a solute dissolving in a solvent. With an ionic compound dissolving in water, the overall energy change is the result of two processes (the energy required to to break the ionic bonds between the ions in the lattice structure, and the energy released when the free ions form dipole attractive forces with the water molecules). Heats of solution are generally measured in an insulated container, called a calorimeter. The process of the dissolving solute either adds or subtracts heat from the solution. The amount of enthalpy change can be determined by using the equation, q=m•C•∆T, with the specific heat of the solution generally being the same as that of water, 4.18 J/g•C°. …show more content…
As the experiment continued (at approximately 90 seconds), the temperature plateaued at approximately 19.75 degrees Celsius.
Evaluation:
Our experiment tested the enthalpy change of a cold pack solid when it reacts with distilled water. We created our own calorimeter and recorded the temperature of the reaction every 10 seconds to see how it fluctuated with time.
We noticed how the reaction immediately dropped in temperature, from 24.0 degrees Celsius at 0 seconds to 19.6 degrees Celsius at 78 seconds. The temperature began to plateau at 90 seconds at approximately 19.75 degrees Celsius, and stayed consistently around this temperature for the remainder of the monitored 3 minute experiment.
Using precise measurements and exact timing, our results are very reliable and accurate. We completed several trials to confirm precision and used high technology calorimeters to guarantee the utmost accuracy. The quality of our results is very trustworthy based off of the quality of the tools used throughout the experiment, the careful measurements taken, and the precision of replication used for the repetition of
Thermodynamics is essentially how heat energy transfers from one substance to another. In “Joe Science vs. the Water Heater,” the temperature of water in a water heater must be found without measuring the water directly from the water heater. This problem was translated to the lab by providing heated water, fish bowl thermometers, styrofoam cups, and all other instruments found in the lab. The thermometer only reaches 45 degrees celsius; therefore, thermodynamic equations need to be applied in order to find the original temperature of the hot water. We also had access to deionized water that was approximately room temperature.
On the lid of the calorimeter, there were two holes and one was being used for the thermometer, and the second one was left open. This hole could have let heat to escape as the reaction was taking place which would have lowered the final temperature value. These conditions would have led to a lower final temperature value. To prevent even the slightest anomalies in the future, any holes on the calorimeter can be covered by tape or another item that could block the passage. The top of the calorimeter could also be covered with aluminum and this would not only cover the holes but would secure the space under the lid so any heat that may escape would stay within the area due to the aluminum. Aluminum could also be tucked in the space between the lid and the calorimeter to once again lock the heat in. This way, the calorimeter will be more effective and maintain all the heat of the reaction resulting in values that are completely accurate and decreasing even the slightest
By adding fresh cold water it should cool the copper calorimeter. By making sure I do these checks before I do the experiment means that I should be able to get accurate results as the test will have been run fairly and hopefully successfully as there should not have been anything gone wrong. To make sure all the measurements are correct, I will also run checks. These checks when recording the data are. Make sure to check the thermometer to see what temperature the water is at the start, so I am able to see what it has to be when its been heated by 10 degrees.
" This means that therefore the enthalpy change of a reaction can be measured by the calculation of 2 other reactions which relate directly to the reactants used in the first reaction and provided the same reaction conditions are used, the results will not be affected. We have the problem set by the experiment to determine the enthalpy change of the thermal decomposition of calcium carbonate. This is difficult because we cannot accurately measure how much thermal energy is taken from the surroundings and provided via thermal energy from a Bunsen flame into the reactants, due to its endothermic nature. Therefore, using the enthalpy changes obtained in reaction 1 and reaction 2 we can set up a Hess cycle.
In a Styrofoam cup, record the temperature of the 200 ml of cold water. This is 200 g of water, as the density of water is 1 g/ml.
Repeat using the SAME metal sample, but instead with the colder water. Do not record the temperature of the cold water in the calorimeter until immediately before adding the heated metal.
The purpose of the lab was to show the effect of temperature on the rate of
In this lab, I determined the amount of heat exchanged in four different chemical reactions only using two different compounds and water. The two compounds used were Magnesium Hydroxide and Citric Acid. Both compounds were in there solid states in powder form. Magnesium Hydroxide was mixed with water and the change in heat was measured using a thermometer. The next reaction combined citric acid and magnesium hydroxide in water. The change in heat was measured as well. For the third reaction citric acid was placed in water to measure the change in heat. In the last reaction, citric acid was combined with water. The heat exchanged was again measured. It is obvious we were studying the calorimetry of each reaction. We used a calorimeter
In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
would only go as high as 70°C to prevent this happening again. Unfortunately, the experiments for 70°C and 60°C were slightly different. anomalous in themselves, as 60°C had a faster rate of reaction than 70° C. This was most probably an error on my part, perhaps timing that. was too slow or a measurement that wasn't accurate for the 60°C or 70°C for the trials.
This is expressed as Δ +ve (delta positive). If the total energy put in is less than the energy created, then the substance warms up (it is exothermic). This is expressed as Δ -ve (delta negative). I will investigate eight different alcohols using an alcohol or spirit burner, to measure the energy change during burning by measuring the change in temperature of some water held in a container.
Methodology: A plastic cup was filled half way with crushed ice and mixed with four spoonfuls of 5 mL of sodium chloride. A thermometer was quickly placed inside the cup to take the temperature and the
On further cooling the χT curve shows a sudden increase to 1.23 cm3.K.mol-1 at T=21 K followed by a sharp decrease down to 0.71 cm3.K.mol-1 at 5 K. The χT maximum de...
My aim in this piece of work is to see the effect of temperature on the rate of a reaction in a solution of hydrochloric acid containing sodium thiosulphate.