Calorimetry Lab

The objective of the lab is to determine the heat of the reaction between magnesium and hydrochloric acid in the calorimeter. To determine the enthalpy change of the chemical reaction, a calorimeter was placed onto the workbench. A balance was place on the workbench. The calorimeter was placed onto the balance and weighed to be 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature recorded is 21.5 C. 50 mL of 1M of Hydrochloric Acid was placed into the calorimeter. 0.150 grams of magnesium was added into the calorimeter. A chemical reaction had occurred and the observed temperature was 34.5 C. The calorimeter was placed onto the electronic scale and was measured to be 68.738 grams. The used calorimeter were

In experiment’s 2rd trail, a new calorimeter was placed onto the workbench. It was placed onto the electronic scale and weighed 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature was 21.5 C. 50 mL of 1M Hydrochloric Acid was placed into the calorimeter. 0.250 grams of magnesium was placed into the calorimeter. A chemical reaction occurred and the temperature recorded was 43.2 C. The calorimeter was placed onto the electronic scale and weighed to be 68.839 grams. Afterwards, the calorimeter was discarded. In the experiment's third trial, a new calorimeter was placed onto the workbench. It was then placed onto the electronic scale and it weighted 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature recorded was 21.5 C. 50 mL of 1M Hydrochloric Acid was placed into the calorimeter. 0.350 grams were added into the calorimeter. A chemical reaction occurred. The recorded temperature is 51.8 C. The calorimeter was placed onto the electronic scale and the total mass is 68.921 grams. All materials were

By dividing .350 grams of magnesium by the molar mass, 24.305 g/mol, the amount of moles used in the reaction is calculated to be .0144 moles. Afterwards, the following equation, Qrnx= -(M * C * t+ Ccal * t) , is used to determine amount of heat in the chemical reaction. M is determined by subtracting the mass of the calorimeter and its contents after the reaction, 68.921 grams., by the initial mass of the calorimeter, 18.600 grams. After the calculation, M is calculated to be 50.321 grams. t is determined by subtracting the final temperature, 51.8 C, from the initial temperature, 21.5 C. From the calculation, is determined to be 30.3 C. From the background information, Ccal is determined to be 9.30 J/°C and C is determined to be 4.18 J/g°C. By plugging the determined values into the equation, Qrnx= -(M * C *t + Ccal *t ), Qrnx, the heat of the reaction is determined to be -6655.15 J/g(c). Finally, to determine the enthalpy value of the reaction, Qrnx,--6655.15 J/g(c), is divided by the number of moles of magnesium used in the reaction, .0144 moles , the enthalpy value of the determined to be -462162.9