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How to investigate a specific heat capacity of a metal
Lab # 6 calorimetry
How to investigate a specific heat capacity of a metal
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In part one of this calorimetry experiment, the heat gained by the system, the sausage, was lost by the surroundings, the water. This relates to the 1st Law of Thermodynamics that states “energy can neither be created nor destroyed”. In parts two and three of this experiment, the heat generated by the reaction was transferred to the solution. The first the first calculation I had to perform was finding the specific heat capacity of the sausage by using the formula, m_water C_(p,water) 〖ΔT〗_water+m_sausage C_(p,sausage) 〖ΔT〗_sausage=0 that is derived from the formulas q_(water=) 〖-q〗_sausage and q=mC_p ΔT. This value, which is the amount of energy in Joules that it takes to raise one gram of the sausage by 1°C, was then multiplied by the number …show more content…
Then comparing the initial temperature of the water to the temperature after the reaction between various salts has occurred, I was able to determine which salt resulted in an exothermic reaction when combined with water. The NaCl and KNO3 were both endothermic reactions because the final temperature was less than the initial temperature. This means that heat was lost by the surroundings, the solution, and gained by the system, the reaction. MgSO4 was exothermic because its final temperature was greater than its initial temperature, which means that heat was gained by the solution and lost by the reaction. Therefore, MgSO4 was the best salt to use for the heat pack because it was the only salt we tested that released heat. After this, we ran three trials with varying volumes of water in order to find the volume ratio of salt to water that would produce a reaction that could release enough heat to raise the temperature of the solution by about 20°C. From this information, I could find the changes of enthalpy of the reaction, which was able to be a substitute for changes in heat content because the reaction took place at a constant
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.
The researcher conducting this experiment is trying to find out which salt- Epsom, table salt, and sea salt- will increase the boiling point of water the most. Sodium chloride is believed to increase the boiling point of water because when salt is suspended into the water, the sodium and chlorine ions leave the “salt crystals” and mix with the water molecules. (“Why does salt… raise boiling point of water?”, 2009).
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.
water has had equal amounts of time for it to heat up, again I will
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.
Tf-Ti). Next, subtract the initial temperature, 25 degrees from the final temperature, 29 degrees putting the change in temperature at 4 °C. To calculate the heat absorbed by the water in calorimeter, use the formula (q = mCΔT). Plug in 50 mL for (m), 4.184 J for (C) and 4 °C for the initial temperature (ΔT), then multiply.
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.
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
- Temperature was measured after and exact time i.e. 1 minute, 2 minutes, 3 minutes.
Sweating and Heat Loss Investigation Aim To find out whether heat is lost faster over a sweaty body compared to a dry body. Apparatus 2 Boiling tubes 47ml max 2 Measuring jug 50ml max A Beaker 250ml max 2 thermometers Paper towels A kettle to boil water A stopwatch 2 magnifying glasses (8x) 2 corks with a small hole through the centre A test tube rack Preliminary work In my preliminary work, I need to find out how much water to use, whether the tissue should be wet with hot/cold water, how often the readings should be taken, how accurate should the readings be, how many readings should be taken and what my starting temperature should be. My results are as follows. Starting temperature of 40°c Time (secs) Wet towel (°c) Dry towel (°c) 30 36 38.9 60 35 38.5 90 34 37.9 120 33.9 37.5 150 33 37 180 32.6 36.9 210 32.3 36.8 240 31 36.5 270 30.4 36 300 30.3 35.9 Starting temperature of 65°c Time (secs) Wet towel (°c) Dry towel (°c) 30 51.1 53 60 48.2 51.9 90 46.4 51 120 46 50 150 44.3 49 180 42.9 48.4 210 42.6 46.9 240 41.7 48 270 40.2 47.5 300 39.3 47 Starting temperature of 60°c Time (secs) Wet towel (°c) Dry towel (°c)
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.
The last part of experiment 5, was learning about specific gravity and temperature. Specific gravity does not have any units, it is unitless. When measuring for the temperature, we used a thermometer to calculate the Celsius of the water, 10% sodium chloride, and isopropyl alcohol. The specific gravity uses a hydrometer to measure the gravity of the liquids. Using the hydrometer, to figure out the measurements we have to look at it from top to bottom. The water for specific gravity was .998 while the temperature of it was 24
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
Therefore there is a greater chance of a collision between KNO3 and water molecules resulting in a successful reaction. Hypothesis My hypothesis is that the temperature of the water affects the solubility of Potassium Nitrate. As I have already addressed this, as you increase the temperature, you also increase the kinetic energy of each particle; thus increasing the chance of a successful reaction. This means more potassium nitrate will be broken down and dissolved in the water as the temperature increases.
My aim in this piece of work is to see the effect of temperature on the rate of reaction in a solution of hydrochloric acid containing sodium thiosulphate. The word equation for the reaction that will occur in the experiment is: Sodium thiosulphate + hydrochloric acid →, sulphur + sulphur dioxide +. sodium chloride + water ? where the sulphur is an insoluble precipitate.