Spirit Burner Experiment Aim: To perform an experiment in the labs to determine the heats of combustion of selected alcohols and then to use this information and the gathered data from chemical data sources to determine trends in the longer chain alcohols. The Variables that MUST be controlled throughout the experiment are: • The height from spirit burner nozzle to the base of the water filled beaker • Air drafts around the room must be kept to minimum so as to keep the heat on the base of the
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2013/07/09 Lecture Presentation Chapter 5 Thermochemistry John D. Bookstaver St. Charles Community College Cottleville‚ MO © 2012 Pearson Education‚ Inc. Energy • Energy is the ability to do work or transfer heat. – Energy used to cause an object that has mass to move is called work. – Energy used to cause the temperature of an object to rise is called heat. Thermochemistry © 2012 Pearson Education‚ Inc. 1 2013/07/09 Kinetic Energy Kinetic energy is energy an object possesses
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is H = U+ ng.RT or qp = qv + 10. ng.RT Exothermic and Endothermic reactions: H = –Ve for exothermic and H = +Ve for endothermic reaction i.e. evolution and absorption of heat. Eg C+O2 N2 + O 2 11. CO2 + 393.5 KJ‚ H = –393.5 KJ (exothermic) 2NO – 180.7 KJ‚ H
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Initial temperature: 23.9 °C Final temperature: 32.9 °C Change in temperature: 9 °C Q = mc∆t = (80g)(4.19 J/g∙°C)(9°C) = 3016.8 J or 3.0168 kJ ∆rH = n∆rHm 3.0168 kJ = (0.05 mol) (∆rHm) ∆rHm = 60 kJ/mol (2 marks) 2. The accepted molar enthalpy of neutralization of sodium hydroxide is - 57 kJ/mol. Calculate the % difference of the value you obtained from your experiment with this accepted value. Answer: % difference = | accepted –
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[pic] LAB REPORT: MBB 2053 ME THERMODYNAMICS II EXPERIMENT: STEAM PLANT (BOILER) GROUP MEMBERS: LAB SESSION: THURSDAY 25 FEB 2010‚ 0800-1000 hrs REPORT SUBMISSION: MONDAY 8 MAC 2010 GROUP 15 1.0 OBJECTIVE The objective of this experiment is to give an experience on the principle of operation of an actual steam power plant. 2.0 INSTRUMENTATION 1. Ten point Digital temperature indicator 2. Pressure gauges 3. Analogue tachometer 4. Dynamometer with voltmeter
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TMA04 Question 1 In TMA02 I asked my tutor to give me specific feedback on the learning outcome Ky1. I was advised that I should take a little more care with significant figures and scientific notation. There has not been much emphasis on significant figures and scientific notation in TMA04. However I have taken the advice given by my tutor and broadened it to include attention to detail in all areas dealing with numbers within this assignment especially in questions 2 ai) 2ci) & 3bi). Question
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the temperature can be lower. 2. 2. Given: 60C(s) → C60; ΔH = 2320 kJ what is ΔH for the following thermochemical equation? 1/60C(s)>>>> C(s) A) +38.7 kJ B) +2320 kJ C) -129 MJ D) -2320 kJ E) -38.7 kJ E is the correct answer. Since the forward reaction has a positive enthalpy‚ the reverse will have a negative enthalpy. Also we are dealing with 1/60th of the original amount‚ so (2320 kJ)*(1/60 mol)*(-1) = -38.7 kJ 3. Exactly 173.9 J will raise the temperature of 10.0 g of a metal
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calorimeter and the temperature change is recorded over a period of time‚ the enthalpy change of the reaction can be experimentally determined. Assumption 1. Mass of H2O in 100cm3 of CuSO4 solution is 100g 2. Specific heat of solution is 4.18 kJ kg-1 K-1 which is the same as the specific heat of water 3. Heat evolved in the reaction will be absorbed by the CuSO4 solution 4. Maximum temperature that would have been reacted if no heat lost to surroundings can be calculated by extrapolation
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Waals equation: For CO2‚ a = 3.6551 dm6 bar mol-2‚ b = 0.042816 dm3 mol-1 The smallest value Pext can have is P2‚ where P2 is the final pressure of the gas. = 28.8 bar -(28.8 x 105 Pa){(0.750 – 2.00) x 10-3 m3} = 3600 J = 3.60 kJ 3. (a) Calculate the work involved when 2 moles of an ideal gas are compressed reversibly from 1.00 bar to 5.00 bar at a constant temperature of 300 K. (b) Calculate the work done if instead the
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Joshua McMahon IB Chemistry Matt Chase 3A 11/5/14 Finding the Molar Enthalpy Change of sodium bicarbonate by using Hess Law Research Question By using Hess’ Law‚ can the Molar Enthalpy Change of sodium bicarbonate be calculated? Hypothesis If we are attempting to determine the enthalpy change of the thermal decomposition of Sodium Bicarbonate‚ then Hess’s Law will be will be the most effective. Introduction Sodium bicarbonate‚ more commonly known as baking soda‚ has many uses in todays
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