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# IA-Enthalpy Change of Reaction - Zinc and Copper Sulphate.

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Introduction

﻿Chul Ou Lee IB Chemistry 1B ROUGH DRAFT Internal Assessment: Determining An Enthalpy Change of Reaction I. Design Objective: The purpose of this experiment is to determine the enthalpy change for the displacement reaction: Zn(s) + Cu(aq) -> Cu(s) + Zn2+(aq) Introduction By adding an excess of zinc powder to a measured amount of aqueous copper (II) sulfate, and measuring the temperature change over a period of time, you can then calculate the enthalpy change for the reaction by the equation: is the enthalpy change of reaction is the mass of copper (II) sulfate is the specific heat capacity of Copper (II) sulfate solution is the mass of Zn powder is the specific heat capacity of Zn is the temperature change The negative sign is present because the heat gained by the Copper (II) sulfate solution and Zinc is equal to the heat lost by the reaction. The reaction is exothermic and thus the sign would be negative. Materials * Safety glasses and lab coat * Graduated Cylinder * Analytical Balance * Styrofoam cup * Stirring rod * Weighing Boat * Beaker * Spatula * Zinc Powder * 1.00 ...read more.

Middle

t1=126 Step 3: Calculate the Final Temperature f(x)=-0.03028x+70.95 Tf=f(126)=67.14 The change in temperature can be found through: Tf-T1 For the example calculation, 67.14-21.8=45.34 Applying the same means of calculation for trials 2,3,4,5, the results can be seen below. Trials Linear Equation T1 Initial Temperature (+/- 0.1) Final Temperature (+/- 0.1) Change in Temperature (+/- 0.1) Average Change in Temperature 1 -0.03028x +70.95 126 21.8 67.14 45.3 44.18 2 -0.03313x+71 129 22.5 66.73 44.2 3 -0.02336x+ 67.47 99 22.4 65.16 42.8 4 -0.02088x +68.39 107 21.9 65.8 43.9 5 -0.03012x+ 69.52 97 21.9 66.6 44.7 *Calculation of Average Change in Temperature Tavg=45.3+44.2+42.8+43.9+44.7=220.9/5=44.18oC Calculating the Enthalpy Change of Reaction To calculate the enthalpy of reaction, the following equation will be used: =44.18oC =25g =6.08g =4.181 Jg-1oC-1 =0.39 Jg-1oC-1 Hence, -(44.18)((25)(4.181)+(6.08)(0.39)) =-4722.67J Now, we must change the value to he correct form because the value (-4722.67J) is the enthalpy change of the reaction when 25mL of 1M CuSO4 reacts, but we want to find the enthalpy change of the reaction per mole of CuSO4 in kJ/mol. ...read more.

Conclusion

When the temperature probe is located closer to the bottom of the Styrofoam cup, the probe would naturally pick up higher temperature, while when it is closer to the top of the solution, the temperature would be lower. Improvements * Two or more Styrofoam cups, or other cups with better heat retention ability can be used. * A hexagonal stirring rod can be used to minimize the clash between the temperature probe and the stirring rod. * The graph can be stopped for the split second while the lid is open to minimize the impact of the opening of the lid on the graph. Also, a better lid with airtight and temperature retention ability can be used. * Acetone cleaner may be used to clean the equipment due to its high volatility and a dryer could be used to make sure that all equipment are well dried and isolated. * More solution can be used for the experiment, allowing more distance between the bottom of the solution and the top. This way, the temperature probe can have a larger leeway and be placed in the center. ...read more.

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