Determination of Acetic Acid in Vinegar Lab Report

Thermochemistry
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INTRODUCTION

Thermal chemistry was intended to display that chemical reaction and phase changes involve energy. The energy of heat was presented when a change in temperature difference was evaluated. Chemical reactions in a calorimeter were used to determine the amount of heat produced by a reaction. Reactions that absorb heat were noted as endothermic, and reactions that release heat were noted as exothermic. These principals were based off of Hess’s Law. The goal of the experiment was to monitor chemical reactions using a calorimeter to monitor changes in temperature. The changes in temperature were to be used to find the amount of heat released or absorbed.

EXPERIMENTAL

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RESULTS

Calculation Calculation for determination of q: q = ms∆T

Hess's Law-type calculation ΔH = ΔHproducts – ΔHreactants
J = g x [ J / ( g x ° C ) ] x ° C
Calculation for Heat Change q=60g(160g*4.4c) =(60g*4.18J)/4.4j
=1104.56 Joules

CLASS TABLE part I

Result Table Part II A-D

PART Reaction Part A 15ml H₂O+ 25ml NaOH+ 20ml HCl Part B 34ml H₂O+25ml HCL+ 1g NaHO Part C 59g H₂O+ 1g NaOH Part D 10ml H₂O+ 25ml NaOH+25ml HOA PART Initial Tempature Final Tempature Change in Tempature ∆H
Part A 24.2C 30.1C 5.9C 1481.136 J
Part B 24.7C 28.5C 3.8C 0953.952 J
Part C 24.0C 28.4C 4.4C 1104.56 J
Part D 24.8C 30.2C 5.4C 1355.616 J

DISCUSSION

The experiment consisted of taking various amounts of the reactants, putting them into a calorimeter to monitor changes in temperature. The: Initial, Final, and Change in temperature, were used to calculate the amount of energy released or absorbed by using Hess’s equation. The goals of the experiment were met. Part I ended with a chart of all the