Wait a second!
More handpicked essays just for you.
Calorimetry and specific heat lab
Calorimetry and specific heat lab
Calorimetry and specific heat lab
Don’t take our word for it - see why 10 million students trust us with their essay needs.
More handpicked essays just for you.
Calorimetry and specific heat lab
Calorimetry and specific heat lab
Calorimetry and specific heat lab
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Our objective was to pick the best chemical to be used in a hand warm. This chemical had to be cheap, relatively safe, and must raise the temperature by 20oC and no more. We add 6 different chemicals to water we record the inshell temperature and then add one a the 6 chemicals to the water and record the temperature change of the water. We also add cold water hot water together to find how much heat would escape the calorimeter. We found that the calorimeter absorbed 71.1J/oC. Then this information to calculate the energy that was released by all of the chemical reaction.
When the copper is heated, the flame of the bunsen burner changed from blue to green. The colour of the copper metal changed from a shiny reddish-brown colour to a dull gray-brown colour. When the magnesium is heated, it changed from a dull gray metal to a pale white colour. b) 2Mg (s)+ O2 (g) ----> 2MgO (s) Magnesium + Oxygen ----> Magnesium Oxide 2Cu (s) + O2 (g)----> 2CuO (s) Copper + Oxygen ----> Copper Oxide c)Copper
The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.
Thermochemistry What is the specific heat of platinum if 1092 J of heat were released into a calorimeter when it was cooled by 65.2 C A 185 g sample of copper at 98.0 C was added to 102 g of water at 20.0 C in a calorimeter. The final temperature of the copper-water mixture was 31.2C. Calculate the specific heat of copper using this data. How much heat in kJ is required to raise the temperature of 250.0 g of Hg 52.0 C? the heat capacity of Hg is 0.14 J/gC.
To conclude, It was predicted that when the combustion of almonds and marshmallows under a flame calorimeter was tested, the almond would emit a larger amount of energy in comparison to marshmallows. In the final analysis, it was proven that since almonds contain larger, more complex sugars while marshmallows contain much smaller, simple sugars, the almonds would burn longer. Accordingly, the longer the food burned, the longer the water had to absorb the heat exiting the food exothermically, which would eventually increase the temperature of the water. As a result, it has been proven that almonds contain a larger energy content than marshmallows. These results demonstrate that the difference in the energy emitted by the two substances is significant
Intro: Light can act as a wave or a particle, it depends on certain circumstances light can go through. It can interact with different chemicals and telling us what we can see in a solution. Light can show the different types of factors that can occur in the state of the substance such as solid, liquid or gas. Light can be absorbed by objects, which means light must be absorbed by a chemical substance in order for the photoelectric effect to take place. This effect is known for electron being emitted when light is shined upon it and photons may or lose the absorbance.
Sariah 's Science Portfolio Question - How does the amount of a substance affect the rate at which temperature changes? Hypothesis - It could be hypothesized that the more mass of water, there is, the longer it takes to heat up. Materials list - Water, graduated cylinder, 2 cups, thermometer. Safety procedures - Be careful when handling the hot cups; wear shoes that cover your toes; don 't wear dangling jewelry and don 't wear billowing shirts.
Al(s) wire was placed in the solution from the last step and 5 drops of HCl along with a stir bar was added to the beaker and this was stirred on the hot plate. Cu(s) precipitate formed on the wire and the solution turned from clear to cloudy until it eventually become a brownish red color. When the reaction was complete the Al(s) wire was scraped with the stirring rod to get off any residual Copper product. All of the reactions except for reaction 3 were exothermic. This is because each reaction gave
The capillary tube was conjoined with a thermometer and heated. Once all of the alum disappeared from the capillary tube we recorded the temperature. On our first trial we recorded 100℃ Our second trial measured at 96C. The alum has a literature melting point at 92.5℃ so our results were in a fair range to assume our results were correct.
The beaker was placed on the heating element on high heat and was left undisturbed until it began to boil. When the solution reached a rolling boil, the temperature of the water was tested and recorded utilising the same method as the first trial. Two more trials of the 0.5 M mixture were conducted. The experiment was repeated three times more with 11.688 grams of salt to create a 1 M mixture. The experiment was repeated three times more with 17.532 grams of salt to create a 1.5 M mixture.
Heating and Cooling Curves Introduction: Experiments 6 and 7 were concerned with the exchange of heat between a substance and its surroundings when the substance undergoes a change in phase. This transfer of heat was indicated by measuring its effect on the temperature of the surroundings (the water in a calorimeter). No direct measurements of the substance undergoing change were made. In this experiment you will observe, by direct measurement, the effects of cooling and heating a pure substance. In Part I, a pure substance will be cooled (heat removed) at a constant rate.
Solar Cookers Planning Board Theoretical background Explain conduction, convection, and radiation. How are solar cookers used in developing countries? Why will this modification increase the temperature change of the water? Conduction is the process by which heat or electricity is directly transferred through the material of a substance where there is a change of temperature or electrical potential between connecting regions, without movement of materials. Some examples of conduction heat are.
I know this because when one object comes in contact with another object, it loses or gains heat till their temperatures get equal. Which object loses heat and which one gains it, is decided by their relative temperatures. In case of ice and metal, ice has a lower temperature than metal. Therefore, here, ice gains heat from metal till they attain the same temperature and ice melts. Also, metals like copper, gold, and aluminum give off more kinetic energy than any plastic block would.
To change the temperature of something depends on how much mass the object has (IsaacsTEACH). The calorimetry equation is Qcalorimeter = m•C•ΔT and is used to find the energy in a substance (Calorimeters). Enthalpy is the internal energy of the system plus the product of the pressure of the gas (Enthalpy). “Three factors can affect the enthalpy of reaction: the concentrations of the reactants and the products, the temperature of the system, and the partial pressures of the gases involved (if any)
The heating effect is caused by the reaction between the oxygen and the carbon and silicon in