Calorimetry lab manual

Laboratory manual for calorimetry fall cal: calorimetry: determination of heats of solution purpose the purpose of the lab is to measure the heats of.  · Lab 9 Introduction. By the end of this section, you will be able to: Determine whether a reaction is endothermic or exothermic. Determine the best ionic compound of to use in a heat pack for treating frostbite based on your experimental results. Calculate the average heat capacity of your calorimeter. Calculate the specific heat of a metal. J/g °C, and based on the chart in the lab book my unknown salt was Na 2 SO 4. T he average total ∆H s per mole of the unknown salt was J/mol, my standard deviation was ,/5(75).

In this lab, you will do two classic calorimetry experiments: measuring the latent heat of fusion of water, and measuring the specific heat capacities of two different metals. Both experiments will use the same apparatus. Apparatus: Fig. 1 shows the construction of the basic calorimeter. The calorimeter is designed to. E12F-1 Experiment 12F FV 10/1/10 CALORIMETRY AND HESS'S LAW: FINDING ΔH FOR THE COMBUSTION OF MAGNESIUM MATERIALS: 12 oz. Styrofoam cup with lid, thermometer, mL and mL graduated cylinders, weighing boat, M HCl, M NaOH, magnesium ribbon, magnesium oxide, copper wire. Pre-laboratory Assignment: Calorimetry and Hess's Law. Show your work for all calculations. When grams of iron metal are mixed with grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from °C to a maximum of °C. The reaction that occurs is given below.

Calorimetry Calorimetry is the science of using a calorimeter. A calorimeter is a device used to measure the change in heat associated with a chemical reaction. The actual output from a calorimeter is a change in temperature of the reaction medium or a water bath. Lab I - 1 LABORATORY I: CONSERVATION OF ENERGY AND HEAT In labs, you used conservation of energy to determine whether or not the internal energy of a system changed during an interaction. In these labs, you will investigate more closely the behavior of a system’s internal energy. The heat capacity of the calorimeter, C cal, is determined by dividing q cal by the temperature change. For this experiment, the calorimeter used is a simple thermos jar and cover. The heat capacity of the calorimeter accounts for the heat absorbed by the thermometer as well as the heat absorbed by the actual calorimeter.