Heat Of Reaction Lab Report

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Patriciah Mulinge Lab Partners: Rachel Reagan, Heaven Wolde Chem:117 TA Daniella Graf Stillfried Station 2 4/6/17 Heats of Reaction Abstract In Physical Chemistry, the bridge between chemistry and physics, usually begins with the study of thermal energy, otherwise called heat. Most reactions either release or consume energy. This loss and or gain of energy can be referred to as either Endothermic-gaining heat, or exothermic- losing heat. it is imperative that chemists understand thermal energy so that they understand how molecules react. The basis of this lab will be to observe three experiments while the react. This will help with understanding the transfer of heat. This lab contains a total of three separate experiments; the first experiment…show more content…
Then 35 ml of 1.00 M of Sodium hydroxide was measured and set aside. Using the calorimeter, the hydrochloric acid was stirred heartily and its temperature was recorded as the initial temperature. The temperature of the Sodium hydroxide was assumed to be similar because they were both in the same conditions (lab) for the exact amount of time. Next the Sodium Hydroxide solution was added to the hydrochloric acid solution in the cups and stirred until the temperature stabilized. This was recorded as the final…show more content…
The margin of error present in the experiments was 48.14% ,8.50% and 10.45% respectively. The heat reaction between magnesium and hydrochloric acid was -462kJ/mol with a 10.45% margin error likely resulting from inadequate sandpapering of the magnesium strip or inaccurate amounts of HCl From the data collecting, it is determined that there’s a correlation between the literature value and the temperature change. In the first experiment the literature value of the eat change is positive so the change in temperature is expected to be negative. This means that that the final temperature will be less than the initial temperature. It is presented as qsoln-q cal. Calorimeter heat change is equal to temperature change multiplied by the calorimeter heat capacity (Ccal). Experiments two and three both have negative heat neutralization for part 2 (NaOH and HCL) and (Mg and HCl), thus the temperature increases as the reaction moves from initial to final

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