Specific heat conclusion. The purpose of this experiment was to measure the specific heat capacity (Cb) of brass using a calorimeter. 2019-02-03

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Expt 1  Specific Heat of Copper

specific heat conclusion

Our experiment could have used a digital system to reduce the amount of electrical noise and make volts entering the water constant. In this experiment, a weighed amount of copper is heated to a certaintemperature and then quickly placed into a calorimeter which contains a measuredamount of H20 at a known temperature. This accounts for the anomalously low heat capacity of diamond in Table. The experimentally observed low-temperature behavior is more like. The specific heat capacity of water is 4.

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Determining Heat Capacity of Water Lab Answers

specific heat conclusion

Others, like nuclear power, create waste problems. There are a number of reasons why the result gained for brass is inaccurate. Thus, the mean internal energy per mole of the solid is 7. Construct a table or a chart in which data could be properly labeled and read before conducting any measurements. Repeat the above for each metal. Now accompany this by bad capacitors to filter the power, we will have some immense electrical noise. Advanced: Consider discrepancies in terms of random and systematic errors.

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The specific heat

specific heat conclusion

The Materials and Method were the usage of a n caliper, electronic scale, calorimeter was used to measure the length, height, width, and mass of the metals and water only mass. It is clear that, when expressed in normal-mode coordinates, the linearized lattice vibrations are equivalent to independent harmonic oscillators. If no energy escapes from the water-metal system, the heat energy lost by the metal will equal the heat gained by the water. Application of Specific Heat Capacity This chart ranks the specific heat of substances, with water having the highest specific heat. Not surprisingly, there is not a particularly strong resemblance between these two curves, because Debye theory is highly idealized.

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Experiment: Specific Heat of a Metal

specific heat conclusion

In this experiment we will be putting the hot metal in a calorimeter of cold water. In the latter case, the mass involved in the vibration is simply that of the molecule, whereas in the former case the mass involved is that of very many atoms because lattice vibrations are non-localized. The longitudinal mode is very similar to the compressional sound wave in gases. Specific heat capacity is measured by determining how much heat energy is needed to raise one gram of a substance one degree Celsius. Since the notes written by the technicians were inaccurate and unfinished, all of the experiments they had preformed needed to redone and documented correctly. The steps to measuring the mass of water and each metal is also explained, but the most important part is explained with swift steps.

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Specific Heats of Solids

specific heat conclusion

Using other web browsers in the Physics lab will put you at a disadvantage For the Physics lab computers there are special links dynamically loaded under the Microsoft Internet Explorer Favorites. Likewise, temperature decreases as heat is removed. As is well known, diamond is an extremely hard substance, so its interatomic bonds must be very strong, suggesting that the force constant, , is large. We also found that placental mammals had the highest oxygen consumption rates and marsupials had the lowest. It follows that we must cut off the density of states above some critical frequency, say , otherwise we will have too many modes. We were supposed to set this at 6 volts; however, we will never truly have 6 volts. Thus, in the Debye approximation the density of normal modes takes the form 7.

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Lab 2

specific heat conclusion

Discussion Based on the results of the lab it can be seen that the metal in the lab can be identified as lead. The pans must reach high levels of heat to cook the food while the handle must remain cool so that the cook will be able to hold it to put the food in plates. Quite often, it is applied to the metallic elements,where it can be used as a basis for comparing energy absorption and transfer. In order to determine the specific heatof the copper sample, an observable temperature change was needed. This specific bacterium is gram-positive which means that it has a thick, protective peptidoglycan coating. At lower temperatures the specific heats drop as quantum processes become significant. The accuracy of the flashes depends on the power supplied to the Joulemeter.


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Lab for Specific Heat Research Paper

specific heat conclusion

In fact, the spacing between the different vibrational energy levels which scales like is sufficiently large in diamond for the vibrational degrees of freedom to be largely frozen out at room temperature. No one is against alternative fuel sources. Anyway, my explanation of this has nothing to do with volume i will write it later after i see some replies. Materials: -Hot Plate -Two 2 Beakers -Water -Metal Objects -Two 2 Thermometers -Pencil -Paper -Calculator Design: A hot plate is acquired and plugged in and if left to warm up. Many alternatives have been proposed and some used. In the end, the Maganesse was canceled out because the Manganesse was not light gary at all, but the Chromium was light gray.

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Specific Heats of Solids

specific heat conclusion

This was a difference of. Units must be included in the calculation in order to confirm that they reduce to the correct units for specific heat. Do you know that it takes longer to boil some liquids than it does others? Step 3: Having filled the 250ml beaker until it was half full with distilled water 125ml ,now place the beaker of water on a hot plate or a ring stand with wire gauze and usethe Bunsen burner to bring to a boil. We can use the quantum-mechanical expression for the mean energy of a single oscillator, Equation , to calculate the mean energy of lattice vibrations in the Debye approximation. Sound wave frequencies are far lower than the typical vibration frequencies of gaseous molecules. The value I calculated for copper in this lab wasvery close to the value of copper in the table of specific heat. When a piece of Copper Cu is submerged in a sample of water, any heat exchangedfrom the metal to the water will result in a temperature change for the water until bothwater and the Copper sample reach equilibrium.

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