Calorimetry
CALORIMETRY
Abstract:
During the experiment, the group were able to perform the following objectives; to compute the heat capacity of a Styrofoam-cup calorimeter, and also to compute the heat of neutralization of 1.0 M hydrochloric acid and 1.0 M sodium hydroxide, the heat of dilution of concentrated sulfuric acid, and the heat of solution of solid ammonium chloride The sixth experiment was named "Calorimetry" wherein it is the measurement of how much heat is gained or released by a system as a chemical reaction occurs within it. The experiment has subtopics namely; Preparation of the Two Styrofoam-Cup Calorimeters, Determination of the heat capacity of calorimeter 1, Heat of neutralization of 1.0 M Hydrochloric Acid and 1.0 M sodium Hydroxide, and lastly Heat of Dilution of Concentrated Sulfuric Acid. The experiment was done in the allotted time and it was quite difficult for us because of the wide range of equation.
Keywords:
Calorimetry, exothermic, endothermic, and heat capacity
Introduction:
Calorimetry is the measurement of how much heat is gained or released by a system as a chemical reaction occurs within it. The heat lost or gained in a chemical reaction is the heat of reaction. The laboratory device in which quantities of heat can be measured is called calorimeter. There are two types of calorimeter: The bomb calorimeter and the open calorimeter. In a bomb calorimeter, the volume of the system is constant. The heat measured equals the change in the internal energy of the system. In an open calorimeter, the pressure of the system is constant. Heat measurements are made by mixing known amounts of reactants in a calorimeter and letting them react. In an exothermic reaction, the chemical reaction gives off heat to the surroundings. The heat is absorbed by the calorimeter and its temperature rises. In an endothermic reaction, the chemical reaction absorbs heat from the surroundings. The heat is absorbed from the calorimeter and its temperature
Abstract:
During the experiment, the group were able to perform the following objectives; to compute the heat capacity of a Styrofoam-cup calorimeter, and also to compute the heat of neutralization of 1.0 M hydrochloric acid and 1.0 M sodium hydroxide, the heat of dilution of concentrated sulfuric acid, and the heat of solution of solid ammonium chloride The sixth experiment was named "Calorimetry" wherein it is the measurement of how much heat is gained or released by a system as a chemical reaction occurs within it. The experiment has subtopics namely; Preparation of the Two Styrofoam-Cup Calorimeters, Determination of the heat capacity of calorimeter 1, Heat of neutralization of 1.0 M Hydrochloric Acid and 1.0 M sodium Hydroxide, and lastly Heat of Dilution of Concentrated Sulfuric Acid. The experiment was done in the allotted time and it was quite difficult for us because of the wide range of equation.
Keywords:
Calorimetry, exothermic, endothermic, and heat capacity
Introduction:
Calorimetry is the measurement of how much heat is gained or released by a system as a chemical reaction occurs within it. The heat lost or gained in a chemical reaction is the heat of reaction. The laboratory device in which quantities of heat can be measured is called calorimeter. There are two types of calorimeter: The bomb calorimeter and the open calorimeter. In a bomb calorimeter, the volume of the system is constant. The heat measured equals the change in the internal energy of the system. In an open calorimeter, the pressure of the system is constant. Heat measurements are made by mixing known amounts of reactants in a calorimeter and letting them react. In an exothermic reaction, the chemical reaction gives off heat to the surroundings. The heat is absorbed by the calorimeter and its temperature rises. In an endothermic reaction, the chemical reaction absorbs heat from the surroundings. The heat is absorbed from the calorimeter and its temperature