The Enthalpy of Formation of Magnesium Carbonate
The Enthalpy of Formation of Magnesium Carbonate
By: Jessica Miller
T.A: Thomas
Lab Partner: Rebekah Melanson
Thursday Lab
Room 106
Chemistry 1001-A
Due Date: Thursday February 3rd 2011
Abstract
The purpose of this experiment was to determine the enthalpy of formation of magnesium carbonate in a lab setting. This was done using a calorimeter, which was calibrated by adding a known amount of both hot and cold water. Following the calibration of the calorimeter, HCl was placed into the empty calorimeter and then mixed with magnesium and then MgCO3 and the temperature changes were recorded. The heat lost by the hot water is thus equal to the heat gained by the calorimeter. Experimentally, it is difficult to determine the standard enthalpy of formation directly, therefore Hess’ Law is applied and the value is determined indirectly using reactions for the formation of Mg2-, MgCO3, H2O and CO2. These experiments led to the determination that the enthalpy of formation of magnesium carbonate is -1087.53 kJ which led to a percent error of 2.2%.
Introduction
Magnesium Carbonate, MgCO3, is a white solid that occurs naturally as a mineral, as has a variety uses. MgCO3 is used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and even toothpaste. It can also be used as a smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, and an additive in table salt to keep it free flowing (Magnesium Carbonate).
The purpose of this experiment is for one to be able to determine the standard enthalpy of formation of Magnesium Carbonate. Every chemical and physical change is accompanied by a change in energy, which usually occurs in the form of heat. The heat of a reaction, also referred to as the change in enthalpy, is denoted by the symbol H. The enthalpy of reaction is expressed as the heat quantity that is evolved or absorbed when one mole of the reactant is converted to product. This is considered to be exothermic
By: Jessica Miller
T.A: Thomas
Lab Partner: Rebekah Melanson
Thursday Lab
Room 106
Chemistry 1001-A
Due Date: Thursday February 3rd 2011
Abstract
The purpose of this experiment was to determine the enthalpy of formation of magnesium carbonate in a lab setting. This was done using a calorimeter, which was calibrated by adding a known amount of both hot and cold water. Following the calibration of the calorimeter, HCl was placed into the empty calorimeter and then mixed with magnesium and then MgCO3 and the temperature changes were recorded. The heat lost by the hot water is thus equal to the heat gained by the calorimeter. Experimentally, it is difficult to determine the standard enthalpy of formation directly, therefore Hess’ Law is applied and the value is determined indirectly using reactions for the formation of Mg2-, MgCO3, H2O and CO2. These experiments led to the determination that the enthalpy of formation of magnesium carbonate is -1087.53 kJ which led to a percent error of 2.2%.
Introduction
Magnesium Carbonate, MgCO3, is a white solid that occurs naturally as a mineral, as has a variety uses. MgCO3 is used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and even toothpaste. It can also be used as a smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, and an additive in table salt to keep it free flowing (Magnesium Carbonate).
The purpose of this experiment is for one to be able to determine the standard enthalpy of formation of Magnesium Carbonate. Every chemical and physical change is accompanied by a change in energy, which usually occurs in the form of heat. The heat of a reaction, also referred to as the change in enthalpy, is denoted by the symbol H. The enthalpy of reaction is expressed as the heat quantity that is evolved or absorbed when one mole of the reactant is converted to product. This is considered to be exothermic
References: Chemistry 1001 Manual. Mount Allison University, Sackville, N.B. (2011). University of Waterloo, . "Hess ' Law." The principle of conservation of energ. N.p., 2009. Web. 1 Feb 2011. <http://www.science.uwaterloo.ca/~cchieh/cact/c120/hess.html>. University of Florida. "Calorimetry." Chemistry. N.p., 2010. Web. 1 Feb 2011. <http://www.chem.ufl.edu/~itl/2045/lectures/lec_9.html>.