<ul><li><a href="#" data-time="6">Collecting Data for Calculating the Heat Capacity of a Calorimeter
</a></li><li><a href="#" data-time="306">Mg(s) + 2 HCl(aq) &#8594; MgCl2(aq) + H2(g)
</a></li><li><a href="#" data-time="547">MgO(s) + 2 HCl(aq) &#8594; MgCl2(aq) + H2O(l)
</a></li><li><a href="#" data-time="720">Results
</a></li></ul>

enthalpy of reaction

Enthalpy of Reaction and Measurement of Heat by Calorimeter - procedure

Enthalpy of Reaction

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Collecting Data for Calculating the Heat Capacity of a CalorimeterExpand
	This experiment will ...

This experiment will use a constant-pressure calorimeter made of two stacked polystyrene cups, a cardboard lid, and a probe measuring the temperature of a solution in real-time. Polystyrene is a good insulator, so you can assume that no heat is exchanged between the inside and outside of the cups. The calorimeter itself will absorb some heat, which you'll account for by calculating its heat capacity.In the first part of this experiment, you'll add hot water to cold water in the calorimeter and measure the temperature increase. After the experiment, you'll calculate how much heat the hot water lost to the calorimeter, rather than to the cold water. First, put on a lab coat, splash-resistant safety glasses or goggles, and disposable gloves.Make sure that your fume hood is clean and ready to use and that your glassware is clean and undamaged. To begin the lab, stack two polystyrene cups to form the insulated calorimeter vessel. Place a magnetic stir bar in the calorimeter.Now, measure the combined mass of the empty cups and the stir bar on a zeroed top-loading balance. Record this in your lab notebook as the empty calorimeter mass and return to your fume hood. Then, measure 50 milliliters of cold tap water and pour it into the calorimeter.Measure the combined mass, record it in your lab notebook, and bring the calorimeter back to your workstation. Calculate the mass of the cold water, or M_cold, by subtracting the mass of the empty calorimeter from the mass of the calorimeter with cold water in it. Now, measure 50 milliliters of deionized water and pour it into a 150-milliliter beaker.Place the beaker on a hot plate under a thermometer clamp and fix a digital thermometer in the water. Then, set the calorimeter in the center of a small stir plate under another thermometer clamp and cover it with a cardboard lid that has a hole in the center. Now, turn on your data-recording device and configure it to record the temperature over time.Set the data-recording rate to two readings per second and the recording duration to 600 seconds. Insert the temperature probe through the hole in the calorimeter lid and clamp it in place. The probe should always be fixed high enough that you can lift the lid.Now, start the stir motor and increase the rotational speed until the stir bar is stirring steadily in the calorimeter. Once the temperature shown on the data acquisition device stabilizes to within plus or minus 0.1 degrees Celsius, record it in your lab notebook as T_cold-initial. Then, turn on the hotplate and monitor the water temperature with the digital thermometer.While you wait, bring some paper towels to your fume hood. Once the water reaches 60 degrees Celsius, turn off the hot plate. Remove the temperature probe from the cold water, wipe it off, and hold it or clamp it in the hot water.Ensure that the probe does not touch the bottom of the beaker as the temperature reading stabilizes. Then, record the temperature in your lab notebook as T_hot-initial. Then, remove the probe from the hot water, wipe it off, and return it to the calorimeter.Once the temperature reading has stabilized, start data collection and wait for the device to record a few seconds of data. Then, carefully pour the hot water into the calorimeter. Monitor the temperature reading as the hot and cold water mix.Once the temperature reaches a maximum, meaning that the temperature is no longer increasing, continue collecting data for five to six minutes to ensure that you record an equilibrium temperature. Then, stop data collection and name the data calibration'Remove the probe and lid from the calorimeter and set them aside. Now, measure the mass of the water-filled calorimeter on the top-loading balance.Record the mass in your lab notebook and bring the calorimeter back to the fume hood. Calculate the mass of the hot water, or M_hot, by subtracting the mass of the calorimeter containing cold water from the mass of the calorimeter containing mixed hot and cold water. Then, remove the magnetic stir bar from the calorimeter and pour the water down the sink.Thoroughly dry the calorimeter and the stir bar and return the stir bar to the calorimeter before proceeding. This is the first reaction that you will perform in the calorimeter. Here, magnesium metal is oxidized to magnesium 2+and H+is reduced to hydrogen gas.You will continue working in a fume hood because of the hazards associated with the reactants and products of this reaction. Magnesium metal ribbon is water-reactive and flammable. Hydrochloric acid is corrosive and toxic, and hydrogen gas is also flammable.Now, let's continue the lab. Create a new data collection run with the same settings as before. Next, label a 600-milliliter beaker for aqueous magnesium waste, which must be disposed of separately at the end of the lab.Now, go to a central hood to obtain the magnesium ribbon, which is provided in 0.45 to 0.55-gram pre-cut strips. Place one piece of ribbon in a weighing boat and bring it back to your hood. Then, use a paper towel and emery paper to polish the magnesium ribbon, revealing shiny, silvery material.Polishing removes the outer layer of magnesium oxide that forms when magnesium metal is exposed to air. Then, cut the polished magnesium ribbon into 0.5 to 1-centimeter long pieces in the weighing boat. Use an analytical balance and a second tared weighing boat to measure the precise mass of your magnesium.Record the mass in your lab notebook. Then, discard the extra weighing boat and bring the magnesium pieces back to the fume hood. Now, bring a 150-milliliter beaker and a watch glass to the fume hood for dispensing HCl, and carefully pour about 110 milliliters of 2.0 molar HCl into the beaker.Cover the beaker and transport it back to your hood. Use a 50-milliliter graduated cylinder to add 100 milliliters of 2 molar HCl to the dry calorimeter. Record the total volume of HCl added and neutralize any drops of spilled acid.Then, put the calorimeter on the stir plate, cover the calorimeter, and clamp the temperature probe in place. Set the stir motor to a medium high speed and start recording temperature data. Wait for 30 seconds of data to be collected so that you obtain an accurate initial temperature.Then, lift the cardboard lid and add the magnesium pieces to the calorimeter all at once. Adjust the stir speed so that the pieces are stirring briskly. It's important to stir the mixture well to dissolve as much magnesium in the acid as possible.Now, close the calorimeter and monitor the data readout as the temperature increases. Once the temperature reaches a maximum, allow data collection to continue for another five minutes. Then, stop data collection and turn off the stir motor.To avoid cross-contamination in your next experiment, thoroughly rinse the temperature probe with deionized water and collect the rinse in the waste beaker. Then, remove the calorimeter from the stir plate and retrieve the stir bar with forceps. Clean the stir bar and forceps in the same way.Now, pour the contents of the calorimeter into the waste and thoroughly wash the calorimeter with deionized water. Dry the calorimeter with paper towels. Switch the stacking order of the polystyrene cups to provide a clean inner surface for the next reaction.Lastly, dry the forceps, stir bar, and temperature probe and return the stir bar to the calorimeter. Here is the second reaction that you will perform in the calorimeter. This is an acid-base reaction in which magnesium oxide neutralizes HCl.As before, magnesium chloride will remain in solution as solvated ions. Magnesium oxide is a respiratory irritant, so use caution when measuring it out. Now, create a new data collection run with the same settings as before to continue with the lab.Then, measure out approximately one gram of magnesium oxide on an analytical balance and record the precise mass in your lab notebook. Next, use your 150-milliliter beaker to transport about 110 milliliters of 2 molar HCl to your fume hood. Pour 100 milliliters of HCl into the calorimeter and record the HCl volume in your lab notebook.Now, set up the calorimeter on the stir plate in the same way as the last experiment. Begin stirring at high speed and start collecting temperature data. Wait 30 seconds to establish an accurate initial temperature reading.Then, lift the calorimeter lid and pour the magnesium oxide into the calorimeter all at once. Ensure that the mixture is stirring vigorously before replacing the lid. Monitor the temperature reading as it increases.Once the temperature reaches a maximum, collect five more minutes of data. Then, stop data collection and turn off the stir motor. Save your data and transfer the file to a computer or flash drive so you can process it later.Now, clean and dry the probe, stir bar, and forceps in the same way as before. Pour the reaction mixture into the waste beaker and rinse the inside of the calorimeter before you dispose of the cups. Then, neutralize the acidic magnesium waste with baking soda, confirm that the pH is acceptable with pH paper, and pour it into a container designated for aqueous magnesium waste.Thoroughly rinse the beaker with deionized water and pour the rinse into the waste. Close the waste container when you are finished. Then, put away your lab equipment and wash your glassware according to your lab standard procedures.Neutralize any non-magnesium-containing aqueous acidic waste with baking soda before flushing it down the drain. Discard the weighing boats, emery paper, and cups appropriately for your lab. Lastly, clean up spilled materials in your fume hood and throw out used paper towels and other trash.First, plot your three sets of data with temperature on the y-axis and time on the x-axis. Now, let's find the changes in temperature that you need for your calculations, starting with your calibration data. You measured the initial hot and cold temperatures directly, so you only need to find T_final, which is the peak stable temperature after the water mixed.Fill in the initial and final values and solve to get delta T_hot and delta T_cold. Next, let's look at the data from your reactions. As with the calibration data, T_final for each reaction is the peak temperature.T_initial is the stable temperature before each reaction began. Fill in these values and solve to get delta T for each reaction. Since delta T is a temperature difference and degrees Celsius and Kelvin have the same interval, you can just change the units to Kelvin.Now, let's calculate the heat capacity of your calorimeter and the changes in internal energy of the reactions. For these calculations, let's assume that the pressure was constant, the volume of the solution barely changed as it heated, and that there was no transfer of energy between the solution and its surroundings. Under these assumptions, the enthalpy change is equal to the heat, which in turn is approximately equal to the change in internal energy.First, let's calculate the heat capacity of your calorimeter. Start by filling in the masses of the hot and cold portions of water from the first part of the lab. Now, fill in the delta T_hot and delta T_cold values that you calculated from your calibration data.Fill in the specific heat capacity of water at ambient pressure and solve to get the heat capacity of your calorimeter. Next, let's calculate the internal energy of the first reaction that you performed. First, determine the mass of your solution by adding together the masses of your reactants.Delta T comes from your graph. You know the heat capacity of your calorimeter and the specific heat capacity of 2 molar HCl is about 3.98 joules per Kelvin gram. Fill in these values and solve to find the internal energy, and thus the approximate enthalpy of this reaction.Use the same process to estimate the enthalpy of the second reaction. Next, for each reaction, identify the limiting reagent and calculate the theoretical yield in moles. Based on this, scale the enthalpies for a yield of one mole.Now, calculate the enthalpy of formation of magnesium oxide using these values and the known enthalpy of formation of H2O. Note that your second reaction must be reversed for these three reactions to add up to the formation of magnesium oxide, so you'll use the negative entropy of the forward reaction. Finally, calculate the percent error between your calculated value and the known enthalpy formation of magnesium oxide.

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Entalpia de Reação

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of 2.0 M Hydrochloric AcidExpand
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lab manual sub articles

18.6K visualizações.  Este experimento usará um calorímetro de pressão constante feito de dois copos de poliestireno empilhados, uma tampa de papelão e uma sonda medindo a temperatura de uma solução em tempo real. O poliestireno é um bom isolante, então você pode presumir que nenhum calor é trocado entre o interior e o exterior dos copos. O próprio calorímetro absorverá um pouco de calor, que você contabilizará calculando sua capacidade de calor. Na primeira parte deste experiment...

Vídeo: Entalpia de Reação - Procedimento