Calorimetry is the measurement of heat transfer. Devices that measure the amount of heat released or absorbed during a process are called calorimeters. Coffee cup calorimeter is the simplest calorimeter and it is often used to measure the heats of chemical reactions at constant pressure (also called enthalpies). This calorimeter consists of a Styrofoam cup with a plastic lid and a thermometer. In today's workshop, we will use calorimetry to calculate the standard molar enthalpy of reaction or the enthalpy change that occurs in a system when 1 mole of matter is transformed by a chemical reaction at 1 atm: AH = qrxn (in J/mol, at constant pressure and pV-work only), where q = cmAT Let's consider the following chemical experiment: A student wants to measure the heat of neutralization reaction. To do this they mixed in a coffer cup calorimeter 58.0 mL of 0.50M HCl solution and 42.0 mL of 0.60M NaOH solution both at 22.0C initially. They then continued to measure the temperature of the mixture for 10 minutes. 1. Write a chemical equation, a complete ionic and a net ionic equations for this reaction. Chemical equation:. Complete ionic equation: Net ionic equation: 2. Discuss with your group the following questions: (a) What is (are) the product(s) of this reaction? Please explain your answer (b) What is the system in this experiment and what are the surroundings? (c) Is this system an open one, a closed one or an isolated one? (a) Now write your answers below and don't forget to explain them. Explain: (b) The system: _is(are) the product(s) in this reaction. The surroundings: (c) We can consider this system to be an system, because: General Chemistry II 3. Now calculate how many moles of product were produced in this experiment.