Enthalpy‚ represented by the sign ∆H in kJ/mol‚ is the heat change in a reaction. It shows whether how much heat is released or absorbed during the reaction. If the reaction is endothermic‚ the enthalpy would be positive and if the reaction is exothermic‚ the enthalpy would be negative. During a chemical reaction‚ which consists of breaking and creating bonds‚ heat is either absorbed or released. In this lab‚ the reaction uses the disassociation of an ionic compound ammonium nitrate shown in the
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Calorimetry: Enthalpy of Neutralization Introduction: The purpose of this lab experiment was to determine the molar concentration of the unknown HCl by using a coffee cup calorimeter. A coffee cup calorimeter is made of Styrofoam cups with a thermometer that is placed from the top and into the calorimeter to measure the temperature as the reaction happens. The Styrofoam cup used for the calorimeter creates an isolated system as it acts as a heat insulator between the cup and the surrounding
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Experiment 1: Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature
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Calorimetry To determine the specific heat of a metal and its approximate atomic mass. To determine the heat of neutralization for a strong acid-strong base reaction. To determine the quantity and direction of heat flow for the dissolution of salt. Post Lab Questions and Answers: 1. In parts A and B in‚ the calorimeter‚ although a good insulator‚ absorbs some heat when the system is above room temperature. Is the reported value for the specific heat of the metal too high or too low? Explain
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MADALANG‚ Kyle Marron A. kyle.madalang@yahoo.com E302: Heat and Calorimetry METHODOLOGY The experiment was conducted following a two part procedure as follows. In the first part‚ the procedure aims to determine the specific heat of metals‚ specifically‚ the brass and aluminum‚ both undergone the following procedure‚ irrespective of their kind to which shall be used first. First‚ the mass of the metal ()‚ the inner calorimeter () and the water () in the calorimeter in grams was determined through
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Experiment: Calorimetry Laboratory Experiment – Heat of Solution Aim: The aim was to use calorimetric measurements to calculate the molar heat of solution of NaOH and NH4NO3. Method: 1. 50g of water was poured into a clean polystyrene calorimeter (Styrofoam cup) and the initial temperature was measured. 2. A teaspoon of 2g of the selected salt was measured and added into the water. 3. The solution was stirred and the final temperature was measured when the solution stabilised and the results
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Date: 16/01/2013 Title: To investigative the Energy Content of Different Foods. Identifying the problem: The energy content of a food sample‚ of known mass‚ was investigated by using a single calorimeter and the word equation below: Heat energy (J) = Mass (g) x Specific heat capacity of water (4.25/g°C for water) x Change in temperature (°C). Dividing the resulting energy value by grams of food burned gives the energy content (in J/g). I predict that that the Brazil nuts
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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
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Heat of Formation of Magnesium Oxide Objetive: To determine the heat formation of MgO (Magnesium Oxide) using Hess’s Law‚ which states the heat within a chemical reaction is independent of the pathway between the initial and final states. Introduction: Chemical reactions require heat energy to complete‚ called an endothermic reaction‚ or produce heat energy‚ and thus called an exothermic reaction. The heat energy produced by such reactions can be measured using a calorimeter‚ a piece
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F6/7 Chemistry Practical: Enthalpy of hydration of copper(II) sulphate Objective: To determine the enthalpy of hydration of copper(II) sulphate Group size: Individual Introduction This experiment enables an approximate determination of the enthalpy of hydration of copper(II) sulphate to be made. The enthalpy change when one mole of anhydrous copper(II) sulphate is dissolved in water is first determined. Secondly‚ the enthalpy of solution of copper(II) sulphate pentahydrate in water is determined
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