PRE-LAB 9: CALORIMETRY SIMULATIONS INTRODUCTION: At its core, a calorimeter is a thermally insulated container that energy (in the form of heat) cannot cscape from. Most are constant volume so there is no work done. The calorimeter represents the surroundings in a thermochemistry experiment. The calorimeter always contains a thermometer so measurements are being made in the surroundings. The system of interest is always placed inside the calorimeter. Heat emitted from or absorbed by the system changes the temperature of the surroundings and is registered on the thermometer. In this lab we will be using a calorimetry simulation by Pearson: hitps://media.pearsonemg.com/bc/bc_Omedia_chem/ chem_sim/calorimetry/Calor.php PART 1: the specific heat of metals. In this part the system will be a piece of solid metal which will be heated. The calorimeter will contain cold water. When the hot metal is placed into the cold water heat will be transferred from the metal to the water. The thermometer reading will track of the heat absorbed by the surroundings. PART 2: heats of solution. When this lab is done in-person we examine the reactions used in hot and cold packs. We will do the same thing here. When you open the simulation you will see a beaker on a hot plate on the left (system) and a calorimeter on the right (surroundings). Under each is a set of tabs: LIQUIDS, SOLIDS, SOLUTIONS where you can choose what type of material will go into the beaker or the calorimeter. Within each tab you can choose the identity of the substance from a drop down menu, its mass (g) and the Temp (oC) for this material