# Specific heat of a metal lab conclusion. Lab Report #11 2022-12-21

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In a specific heat of a metal lab, students are tasked with determining the specific heat capacity of a metal by measuring the temperature change of the metal as it absorbs heat from a hot water bath. The specific heat capacity of a substance is a measure of how much heat is required to raise the temperature of a given mass of the substance by a certain amount.

To perform the lab, a student would first measure the mass of the metal sample and the temperature of the hot water bath. The metal sample is then placed in the hot water bath, and the temperature of the metal is measured at regular intervals until it reaches the same temperature as the water.

Using the data collected, the student can then calculate the specific heat capacity of the metal using the formula:

Q = mcΔT

where Q is the amount of heat absorbed by the metal, m is the mass of the metal, c is the specific heat capacity of the metal, and ΔT is the change in temperature of the metal.

The results of the lab can be used to compare the specific heat capacities of different metals, as well as to understand how different materials absorb and transfer heat. For example, a metal with a high specific heat capacity will require more heat to raise its temperature, but it will also be able to absorb and retain more heat before its temperature begins to rise.

Overall, the specific heat of a metal lab is a valuable tool for understanding the properties of different materials and how they interact with heat. It allows students to gain a deeper understanding of the science behind heat transfer and the factors that influence it, which can have practical applications in fields such as engineering and materials science.

In a specific heat of a metal lab, the specific heat of a metal is determined by measuring the temperature change of a metal sample as it absorbs a known amount of heat. The specific heat is the amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius.

In this lab, a metal sample is placed in a calorimeter, which is a device used to measure the heat transfer between substances. The metal sample is heated to a high temperature using a flame, and the temperature of the metal is measured using a thermometer. The metal sample is then placed in a known mass of water at a lower temperature, and the temperature of the water is measured as the metal sample transfers heat to the water.

From the temperature change of the metal and the water, the heat absorbed by the metal can be calculated using the equation Q = mcΔT, where Q is the heat absorbed, m is the mass of the substance, c is the specific heat, and ΔT is the change in temperature. By dividing the heat absorbed by the metal by the mass of the metal and the change in temperature, the specific heat of the metal can be calculated.

In conclusion, the specific heat of a metal can be determined by measuring the temperature change of the metal as it absorbs a known amount of heat and using the equation Q = mcΔT. This information is useful in a variety of applications, such as predicting the heat capacity of a substance and understanding how different materials conduct heat.

## The Specific Heat of Different Metals: A Comparative Experiment: [Essay Example], 686 words GradesFixer

Heat flows between the system and surroundings until the two are at the same temperature, when a chemical reaction occurs in which the system absorbs heat, the process is endothermic it feels cold. This explains why energy cannot be created nor destroyed. Mathematically, my hypothesis was completely accurate although using the data from the lab; I could not conclude my hypothesis was correct. Quickly remove a test tube from the heated beaker and place the metal into the calorimeter. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter. The balance used only rounded to the hundredths place and the thermometer only rounded to the tenths place. The first law of thermodynamics states that matter or energy can not be created nor destroyed.

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## Lab for Specific Heat

Find the temperature of the heated water then record on data table Heated Metal Temp. Our most accurate calculation was when we tested Copper. This explains why energy cannot be created nor destroyed. He is credited with the invention of a calorimeter used to measure precise heat quantities in substances. Richards received his PhD from Harvard in 1888. Make sure the thermometer is in the water and find the temperature then record it on the data table Room Temp Water.

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## Specific Heat Lab Report

Place a big styrofoam cup inside the other big cup and place 50mL of water in the stacked cups. The specific heat of a substance represents the amount of heat required to raise a particular mass of a substance through a particular temperature difference. This resulted in a 22. This may have changed our results. An instrument called a calorimeter is used to measure specific heat. If the aluminum balls are heated in the test tube and poured into the water in the plastic foam cup, then the specific heat calculated from both trials will be precise because the accepted value for the specific heat of aluminum is independent from the mass of aluminum or water used. Then place the stacked little cups upside down on top of the big stacked cups.

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## Formal Lab Report Example (Specific Heat)

Weigh Calorimeter again with the cold water. He was awarded the Nobel Prize in Chemistry in 1915. It is also believed, however, that the specific heat measured by the calorimeter will not be accurate compared to the verified data. We used a few different metals for this experiment. More importantly, the procedure did not request an amount of time for the aluminum in the boiling water. Additionally, there was a bigger increase in temperature change of aluminum in trial 2 because there was a smaller increase in the temperature of water in trial 2. Last calculate the percent error and record the data.

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## Specific Heat Lab Conclusion

While this is boiling, fill an insulated container with room temperature water. The first law of thermodynamics states that matter or energy can not be created nor destroyed. Next place the little styrofoam cup in the other little cup. Add 70 mL of cold water from the tap into the Calorimeter. Overall, our results were relatively accurate and weremathematically what I predicted. Place each unknown metal into a test tube then place them into the beaker that is being heated. The possible errors in this lab include the errors that occurred in the weighing scale that was used ie.

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## Specific Heat of Metal Lab

It would have been possible to my hypothesis was correct with the data if I had more constants. The density of the unknown metal was 6. Carefully measure the water's temperature and record it in your data table. When we did the specific heat test for Tin, we were only 0. Find the temperature of the heated water then record on data table Heated Metal Temp.

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## Specific Heat of Aluminum: Lab Report on Testing Experiment: [Essay Example], 1319 words GradesFixer

The reason for this could be because Sample 2 weighed the most while the other two samples were similar in lighter weight. In addition, the thermometer had an error of ± 0. Theory Specific heat is the amount of energy required to raise the temperature of one gram of a substance by one kelvin The lab uses the specific equation in two separate ways: first to find the heat gained by water and then the specific heat of the aluminum. Weigh the Calorimeter again with the cold water in it and record it. My hypothesis was that the metals specific heat and the final temperatures were directly proportional. The piece of metal is then taken out of the boiling water and placed in a calorimeter which contains room temperature water. Once it has reached a peak in temperature, record the results Record the results for each trial when changing metals.

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## Lab Report #11

The study of specific heat falls under the category of Thermochemistry which is further divided into the category of Calorimetry. Then place the stacked little cups upside down on top of the big stacked cups. Record this in your lab notebook. If we had done more trials I think the percentage of error would have decreased. Plug in all data into the formulas and find the specific heat of each metal. Using the calculations from the lab, the students were then able to calculate the actual specific heat obtained from the lab and compare it to the accepted value.

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