CALORIMETRY WORKSHEET (VIRTUAL Experiment), Lab Reports of Chemistry

Download CALORIMETRY WORKSHEET (VIRTUAL Experiment) and more Lab Reports Chemistry in PDF only on Docsity! EXPERIMENT No.1 CALORIMETRY(VIRTUAL) OBJECTIVES • To carry out basic calorimetry experiments. • To compute the specific heat of an unknown metal using calorimetry results. • Calorimetry measurements were used to determine the heat of reaction (H). INTRODUCTION The two most prevalent ways for a system to exchange energy with its environment are heat and work. In reactions that do not involve gases, the work term is zero, therefore all of the energy change is converted to heat. Calorimetry is a technique for determining the quantity of heat that flows into or out of the environment (heat measurement). An insulated container, a thermometer, a mass of water, and the system to be investigated make up a calorimeter. To put it another way, we can say that the thermodynamic universe is made up of the system and the water that surrounds it. We'll put this theory to the test in the experiment. Calorimetry is a technique for determining how much thermal energy is transmitted during a chemical or physical reaction. This necessitates meticulous monitoring of the temperature change that occurs during the operation, as well as the masses of the system and its surroundings. The advantage of calorimetry is that it is fully non-specific, which means that it may be used to measure practically any form of biological reaction or activity. The instrument's sensitivity could be the limit. Calorimetry is a vital tool in biological research. Calorimetry is a frequently used chemical reaction and biochemical reaction measurement method. The fundamental benefit of calorimetry is that it does not require complicated equipment and can monitor very small energy changes. Calorimetry can be applied in a variety of fields, including life science, clinical medicine, pharmacology, biotechnology, ecology, environmental research, and many more. CONCEPTS • Calorimetry is the science or act of determining the heat transfer associated with changes in a body's state owing to chemical reactions, physical changes, or phase transitions under specified restrictions by measuring changes in state variables. • Calorimetry is a technique for determining how much heat is generated or absorbed during a chemical reaction. It is possible to identify whether a process is exothermic (releases heat) or endothermic (stores heat) by measuring the change in heat (absorbs heat). Calorimetry is also used in everyday life to control metabolic rates in humans and, as a result, to maintain functions like body temperature. MATERIALS • In the video that was shown to us, the materials that are needed in the calorimetry experiment are composed of an insulated container, a thermometer, a mass of water, and the system to be studied. The use of an insulated container (Styrofoam cup in this experiment) allows us to assume that there is no heat transferred through the calorimeter walls. PROCEDURE • Place the thermometer in the calorimeter cup and record the temperature for 3 readings at 30 second intervals • Lift the lid of the calorimeter and drop the pieces of magnesium in, mixing continuously. • Record the temperature every 30 seconds until 10 minutes have elapsed. In a water bath, a typical calorimeter simply captures all of the energy emitted (or absorbed) by a process. We can quantify the heat (enthalpy) of the chemical reaction by measuring the change in water temperature. DATA SHEET 1 = -58,391,175 J/57.99g(201.85 K) (∆T)metal = -71.3 °C = -58,391,175 J/11,705,29 g(K) (q)metal = -58,391,175 J (c)metal = -4,988,447J/g(K) Solution for Metal 2(Zinc) (q)water = (-q)metal (q)water = [(m)water][(c)water][(∆T)water) = (50 g)[4,182 J/g(K)](279.55 K) (q)water = 58,453,905 J Thus, (q)metal would be -58,453,905 J Formula for finding the (c)metal: (c)metal = (q)metal/(m∆T) = -58,453,905 J/57.97 g(202.15 K/) = -58,453,905 J/11,718.636 g/K (c)metal = -4,988.115 J/g(K) Finding the (%)Error: Formula: (%)Error = Theoretical Experimental/Theoretical(100) = [0.387 J/g(K) - (-4,988.115 J/g(K)/0.387. J/g(K)](100) = [4,988.502 J/g(K)/.387. J/g(K)](100) = 12,890.186(100) (%)Error = 1,289,018.6 Solution for Metal 3(Tin) (q)water = (-q)metal (q)water = [(m)water][(c)water][(∆T)water) = (50 g)[4,182 J/g(K)](277.55 K) (q)water = 58,035,705 J - Thus, (q)metal would be -58,035,705 J Finding the (c)metal Formula: (c)metal = (q)metal/(m∆T) = -58,035,705 J(57.93 g)(199.55 K) = 58,035,705 J/11,559.932 g(K) (c)metal = -5,020.419 J/g(K) Finding the (%)Error: Formula: (%)Error = Theoretical Experimental/Theoretical(100) = [0.227 J/g(K) - (-5,020.919 J/g(K)/0.227 J/g(K)](100) = [5,020.646 J/g(K)/.227 J/g(K)](100) = 22,117.383(100) (%)Error = 2,211,738.3 CONCLUSION In conclusion, calorimetry is a technique for determining how much heat is transferred between two states or environments as a result of chemical and physical changes. Calorimetry is significant because it is used to calculate temperature changes based on how much heat a system gains or gives in a response. The advantage of calorimetry is that it is fully non-specific, which means that it may be used to measure practically any form of biological reaction or activity. The instrument's sensitivity could be the limit. DOCUMENTATIONS SOLUTION FOR METAL 1 (COPPER)