100g Brass Mass And Calorimetry Lab Results

The water was transferred to a 400mL beaker. The beaker was transferred to a hot plate to boil the water. A Styrofoam cup, a plastic pipette and a scale were used to measure about 150g of room-temperature deionized water. The water was transferred to the coffee cup located in the calorimeter. The initial temperature of the water was measured using a thermometer, which was allowed to equilibrate with the water for a few minutes first and then the temperature was recorded.

Mathematically and scientifically, using Albert Einstein’s most famous equation, E = mc2, states anything which has a mass has the equal amount of kinetic energy proving they can be changed into each other and therefore if heat is added to corn syrup the mass would change since the heat is the energy. At the end of the experiment once the procedure was followed and complete, the results which were found was there were no experimental errors which had occurred, however, there could have been something that went the way it was not supposed to. Some of the experimental errors that could have affected the results could have been the stopwatch being started late giving inaccurate information, which further on impacts when finding the average, it could have been remarkably smaller or larger than what it should have been. Also, a misconception could be that the substance was placed longer than it should have been in either the cold or hot water bath impacting the water particles and creating a difference when determining the flow rate as it could have been faster than what was

Ø Firstly I am going to measure out 100cm3 cold water, using the measuring cylinder (so that the water I put into the calorimeter is accurately measured out) rather than using an ordinary beaker, as an ordinary beaker is less precise compared with a measuring cylinder.

For q, you found how much heat was gained by the water so you know that same amount of heat was lost by the metal. Therefore, qmetal = -qwater. The mass of the sample was recorded from the baggie. The temperature change

Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

When the temperature changes so does the results. The blue stick, hot water, stayed lit for 112 minutes (an hour and fifty-two minutes). The green stick, which was room temperature water, stayed lit for 96 minutes (an hour and thirty-six minutes). And lastly, the pink stick, in cold water, stayed lit the longest for 122 minutes (two hours and two minutes).

Is it possible to find the specific heat of unknown metals using calorimetry? This experiment was designed to determine the specific heat capacity of two unknown metal sample. By comparing the data with the accepted heat capacities of various metals, the composition of the unknown samples was identified. Two unknown metals were put in boiling water for two minutes to ensure thermal equilibrium. The metal was then transferred into a calorimeter where the temperature was measured. The steps above were repeated for the second unknown metal as well. The cp , specific heat, of the metal was then calculated. Based off of the calculations, the obscure metal number one is zinc. This is on the account that the specific heat of the unknown metal was

The second experiment involved the heat exchange between metal and water. The metal in beaker and water in calorimeter

Objective: The objective of this experiment was to discover the specific heat of an unknown metal. By heating a metal then placing it in a calorimeter and taking the temperature of the solution as the heat transfer from the metal to the solution. This is done using a calorimeter, thermometer, 2 200mm test tube, an unknown metal, hot plate, 2 50ml graduated cylinders, sodium hydroxide, and hydrochloric acid. The techniques that are used in this experiment is cleaning glassware, disposing of chemicals, measuring mass, transferring solids, transferring liquids and solutions, heating liquids and solutions, and measuring the volume of solutions by examining the meniscus. Introduction: Chemical reactions always exerts some form of thermal energy, that energy then applies changes to its reactants, this is called Calorimetry which is the analysis of temperature change or heat change within a chemical reaction.

Task 1 Hypothesis By increasing the mass of substance using 20ml of water starting at room temperature there will be 10oc change, either an exothermic change or an endothermic change. Aim The aim of this investigation experiment is to find out what mass of substance is required for an exothermic or endothermic substance to achieve a 10oc temperature change. Set objectives • 7 masses of each substance should be used in this experiment: 0g, 0.25g, 0.50g, 0.75g, 1.00g, 1.25g, 1.50g, 1.75g, and 2.00g. • Measure the start and end temperature for each substance using a thermometer.

This experiment will show the connection between temperature the chemiluminescence of light sticks. How will the temperature in each cup effect the chemiluminescence of the sticks and which temperature will add and remove more energy to the chemical reaction in each light stick. The independent variable in this experiment will be the temperature in each cup which will be measure in degrees, the dependent variable will be the reaction of each light stick and the constant will be that the light sticks will be the same, same cups, same thermometers and the light sticks will stay in the cups for the same amount of time.

(21.0 + 23.9 + 18.1) / 3 = 21.0g Average weight of evaporating dish before heating= = (17.73 + 17.85 + 18.61) / 3 = 17.73g Calculation to find Molecular Formula for Hydrate of Copper (II) Sulphate, CuSO4, XH2O Mass of Evaporating dish = 17.73g +- 0.05 Mass of Evaporating dish + Blue Copper Sulphate = 21.85 +- 0.05 Mass of Blue Copper Sulphate = 21.00g +- 0.05 Mass of White Copper Sulphate = 4.12g +- 0.05 Mass of H20 = Mass of white Copper Sulphate – Difference in mass of evaporating dish = 4.12 – (21.00 – 17.73) = 1.85g +- 0.05 Moles of White Copper Sulphate=(Difference in mass of evaporating dish)/molar mass

Supplying a thousand grams of energy to water is not the same as supplying a thousand grams of energy to a metal for they will not rise the same when it all comes down to temperature. What the difference is between water and a metal is that they are both of different materials, which is they both would have different boiling and melting point, conductivity and varied structures of and intermolecular bonds of the substances. To calculate the amount of heat energy require for a compound or mixture, the mass of the

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the