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What Are The Specific Heat Of Naoh And The Enthalpy Of A Neutralization Reaction

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In the lab the goal of measuring the specific heat of NaOH and the enthalpy change of a neutralization reaction between NaOH (strong base) and HCl (weak acid) was accomplished. This was accomplished by finding the heat of solution of the salt and measuring the heat capacity of the calorimeter to measure the enthalpy. During this lab one of the assumption that was made was the law of conservation of energy. Specifically, the loss of heat is equal to heat gained. The heat of solution with the assumption no heat loss was -43.884KJ/mol and with the heat loss to the calorimeter was -42.816KJ/mol. This value is not far off from the theoretical value of NaOH, which is -44.2KJ/mol, meaning there was only about a 3% error. When calculating the heat of solution of the salt, a couple of …show more content…

Furthermore, the value attained for the calorimeter constant was 0.1748 KJ/°C, this value allowed to apply the correction for heat loss to the calorimeter. However, during the calculation for the calorimeter constant, the assumption that the specific heat of water was 4.184 J 〖deg〗^(-1) g^(-1). The concentration of NaOH was attained when assuming no heat loss was 0.8170 M and including the heat loss the concentration of NaOH was 0.9493 M. These values are very close to the expected value of the concentration, which is 1.071M considering the experimental error is only about 11 percent off. Based off the values obtained in the experiment compared to the theoretical values, there is a very little experimental error, meaning the method was precise. Therefore, the calorimeter was efficient method of measuring the change in temperature because it allowed chemical and physical process to occur, while being isolated. Some of the errors that may have occurred causing the result not to be as precise, is that our eyes are not a precise measuring

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A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.

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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.

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Then the scientist will observe the different rates of reaction with temperature. The Boltzmann distribution of law, indicates that high temperature makes molecules gain high energy contents (pubs.acs.org/doi/abs/10.1021/ja). In order to measure the reaction rate, the scientists must use the same volume of water at three different starting temperatures: hot tap

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The molar heat of combustion of a compound is 1250 kJ/mole. If 0.115 moles of this compound in a bomb calorimeter with 2.50 L of water, what would the temperature increase be? If change in heat is positive it is an _______ reaction If change in heat is negative it is an_______ reaction

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One way we could improve the experiment is by doing more trials, the more trials the more accurate the resolutes are. Another way we could improve the experiment is to have more time so we could make sure all the temperatures

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723 Words | 3 Pages

With following the procedure, the experiment was completed very easily. The technique used worked very well. The graduated cylinder were dried after each trial to ensure each water level was equal. The air bubble were risen to the top to ensure the equal amount was measured. Systematic errors can not be eliminated by averaging In principle, they can always be eliminated by changing the way in which the experiment was done.

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It is very possible, since all of the components were found that were necessary to use the formula and the date proves that. The data above supports the claim that the specific heat was found by using the formula. The specific heat was 0.345J/g℃ for the iron. Errors could have occurred, such as the thermometer wasn’t left in the calorimeter long enough, which would mean that the final temperature of the water and the metal would be different, which would then mean that there would be a different result for the specific heat of the metal. Another error that could have occurred would be if the metal wasn’t transferred from the boiling water to the calorimetry with the room temperature water quick enough then the metal could have lost heat from the outside environment.

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Next, I had to test the different amount of sodium chloride in the water as I took four 250 ml beakers and labeled them A, B, C and D. Then added 100 ml solution containing 0, 1, 3, and 5, M sodium chloride in the each beaker. After I had set up the tripod and non-asbestos pad over a bunsen burner, I placed the solution from the beakers to the cylinder on the tripod and began to boil each solution one at a time and record the temperatures with the thermometer. The data that I collected is in the chart

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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.

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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.

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The items that were massed were the evaporating dish, watch glass, and NaCO3. The materials were massed once before and once after being heated in the drying oven. The mass of the evaporating Dish before was 46.57 g; while after being heating was 60.15 g. The mass of the watch glass before was 57.97 g and after was 48.75g. There were two masses taken for the substance NaHCO3- one with the evaporating dish and one without, subtracted out after the lab was concluded. The mass of the substance with the dish was 48.79 g before and 62.33 g after; meanwhile, the mass of the substance without the dish was 2.22 g before and 2.18 g after. The mass of the NaHCO3 had changed after the reaction occurred along with after it was placed on the hot plate and being in the drying oven.

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The enthalpy of neutralization between an acid and base in aqueous media could be directly measured by mixing the two regents together in a calorimetry and recording the ΔT.3 Other values are experimentally more difficult (or impossible) to measure, directly.3 Some equations are difficult to find the enthalpy straight off, this is when the use of a calorimetry of two other compounds can be used to then equal the enthalpy of the equation wanted. There are many types of calorimeters that can be used the one used was a Styrofoam one. This what causes some heat being transferred to the calorimeter rather than just staying the

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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)

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1054 Words | 5 Pages

Another way to calculate the enthalpy of neutralization is to assume the density of the solution to be equal to the density of water in order to assume the mass of the solution. 1.00 g 〖cm〗^(-3)×50 cm^3±0.96 %= 50.00 g ±0.96 % The heat released can then be calculated using the assumed mass. q=50.00 g±0.96 % ×4.18 J g^(-1)

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Also, it has played an important part in biology. Antoine Lavoisier is the person who discovered calorimetric measurements on biology applications. Calorimeter is important in biological side because every creature is an energy processing system. Moreover, the analysis of energy in a biological system would give inclusive information about how living thing use energy for growing, reproducing and many different procedures. Every living thing is an open system which means that it should take in and give off operations as side of its normal processes and it is extremely hard to make exact heat –flow estimation on open system.

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