Introduction The porpoise of these is to determine the Specific Heat. Also known as Heat Capacity, the specific heat is the amount of the Heat Per Unit mass required to raise the temperature by one degree Celsius. The relationship between heat and temperature changed is usually expected in the form shown. The relationship does not apply if a phase change is encountered because the heat added or removed during a phase change does not change the temperature. Q = cn^T The molar specific heats of most solids at room temperature and above are nearly constant, in agreement with the Law of Dulong and Petit. At lower temperatures the specific heats drop as quantum processes become significant. The Einstein-Debye model of specific heat describes the low temperature behavior. The metal samples are: · Copper (CU) · Aluminum (Al) · Zinc (ZN) · Tin (Sn) · Lead (Pb) · Steal/iron (Fe) · Brass (an alloy of Zn and Cu) PROCEDURE: 1. 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. 2. Obtain a sample of metal that has been immersed in boiling water and place it in the cup of water. 3. Wait until the temperature no longer rises (thermal equilibrium), and record the temperature increase. 4. Discard the water and measure the mass of the metal. 5. Repeat the above for each metal. CALCULATIONS: 1. H=mc^T=(200g/1)(1cal/goc)(2oc/a)=400cal C=H/m^T=400cal/(128g)(20c)=1.5625cal/goc 2. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(20.1g)(2oc)=400cal/40.2 goc=9.95cal/ goc 3. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(53.9g)(20c)=37.38cal/ goc 4. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(65.3g)(20c)=3.06 cal/ goc 5. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(70.5)(20c)=400cal/141goc=2.83 cal/ goc 6. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(70.1g)( 20c)= 2.83 cal/ goc 7. H=mc^T=(200g/1)(1cal/goc)(2oc/1)=400cal C=H/m^T=400cal/(50g)(20c)=4 cal/goc RESULTS: Type of Metal Experimental © of Metal Actual © of Metal CU 400cal 1.5625cal/goc Al 400cal 9.95cal/ goc ZN 400cal 37.38cal/ goc Sn 400cal 3.06 cal/ goc Pb 400cal 2.83 cal/ goc Fe 400cal 2.83 cal/ goc Brass 400cal 4 cal/goc
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.
As much as 95% of employers favor urine testing as a method for drug testing, and this one piece of statistic may have positively affected the trend and demand for synthetic urine over the years.
Start with the hot water and first measure the temperature. Record it. 8. Then pour 40 ml into the beaker. You can measure how much water was used by looking at the meniscus.
The purpose of this experiment is to try to find the original temperature of the hot water in the heater using the 60 degrees C thermometer. Use your 60°C thermometer, and any materials available in your laboratory, to determine the temperature of the water in the coffee pot. During this experiment we calculated the original temperature of a heater after it had been cooled down, and we did this by measuring hot, cold, and warm water, with a thermometer that had tape covering 60 degrees and up. When preformed each of these experiments with each temperature of water, plugging them into the equation (Delta)(Ti – hot – Tf) T Hot x Cp x Mass(Cold) = (Delta)(Tf – Ti – Cold) T Cold x Cp x Mass(Hot)(d
The purpose of this lab was to calculate the specific heat of a metal cylinder
We must first begin the today’s lab by connecting the thermometer that digitally detects surrounding temperature to the Lab Pro Interface located on the computer via...
4. Pour about 300mL of tap water into the beaker. Set up a hot-water bath using a hot plate, retort stand, and thermometer clamp. Alternatively, use a Bunsen burner, retort stand, ring clamp, thermometer clamp, and wire gauze.
The thermometer, containers, and iron ball were secured of any possible contaminants. The stopwatch was calibrated and checked to be correctly measuring the time in seconds and milliseconds, by comparison with other stopwatches. The thermometer was checked to be accurately measuring the temperature of lukewarm water, and was al...
c- Specific heating capacity of water. m- Mass of water in grams. . T - Change in temperature of water I will then compare the enthalpy changes and the types of molecular structures and so I will be able to out why enthalpy change is affected.
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 how long it takes to heat up. If we heat a large volume of water it
Specific heat capacity of aqueous solution (taken as water = 4.18 J.g-1.K-1). T = Temperature change (oK). We can thus determine the enthalpy changes of reaction 1 and reaction 2 using the mean (14) of the data obtained. Reaction 1: H = 50 x 4.18 x -2.12.
The objective of this experiment was to identify a metal based on its specific heat using calorimetry. The unknown metals specific heat was measured in two different settings, room temperature water and cold water. Using two different temperatures of water would prove that the specific heat remained constant. The heated metal was placed into the two different water temperatures during two separate trials, and then the measurements were recorded. Through the measurements taken and plugged into the equation, two specific heats were found. Taking the two specific heats and averaging them, it was then that
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.
A warm water was prepared by heating approximately 100mL of distilled water in a 400mL beaker along with few boiling chips to 45-50 ℃.