3-5: Heat of Combustion: Chicken FatThe heat of combustion (AHcomb) is the heat of reaction for the complete burning (reacting with O2) of onemole of a substance to form CO, and H,O. Calorimetry experiments that measure the heat of combustioncan be performed at constant volume using a device called a bomb calorimeter. In a bomb calorimeter asample is burned in a constant-volume chamber in the presence of oxygen at high pressure. The heat thatis released warms the water surrounding the chamber. By measuring the temperature increase of thewater, it is possible to calculate the quantity of heat released during the combustion reaction. In thisassignment you will calculate the heat of combustion of chicken fat. The calorimeter has already beencalibrated by combusting benzoic acid.1. Start Virtual ChemLab, select Thermodynamics, and then select Heat of Combustion: Chicken Fatfrom the list of assignments. The lab will open in the Calorimetry laboratory with the bombcalorimeter out and disassembled and with a sample of chicken fat in the calorimeter cup on thebalance. The balance has already been tared.2. Record the mass of the chicken fat sample from the balance. If you cannot read it click on theBalance area to zoom in, record the mass in the data table below and return to the laboratory.3. Double-click the following (in numerical order) to assemble the calorimeter: (1) the cup on thebalance pan, (2) the bomb head, (3) the screw cap, and (4) the bomb. Click the calorimeter lid to closeit. Combustion experiments can take a considerable length of time. Click the clock on the wall labeledAccelerate to accelerate the laboratory time.4.Click the bomb control panel and the plot window to bring them to the front. Click on the Save buttonto save data to the lab book. Allow the graph to proceed for 20-30 seconds to establish a baselinetemperature.5. Click Ignite and observe the graph. When the temperature has leveled off (up to 5 minutes oflaboratory time), click Stop. A data link icon will appear in the lab book. Click the data link icon toview the collected data. Record the temperature before and after ignition of the chicken fat sample inthe data table.Data Tablechicken fatmass of sample (g)initial temperature (°C)28.7274.762Kfinal temperature (°C)6. Calculate AT for the water using AT = |T- T.7. Calculate the moles of chicken fat in the sample (MW ja = 797.7 g/mol).I.0328=1.29X10 moles797.7© Beyond Labz, all rights reserved 8. AHcomb for chicken fat can be calculated using AHomb = (Catem AT)/n, where n is the moles ofchicken fat in the sample and Cystem is the heat capacity of the calorimetric system.Use 10.310 kJ/K for Cstem and calculate the heat of combustion, in kJ/mol, for chicken fat.br chickentit=(( sy stem x 4T)- 5.310 yh76.762-1||950.56%l1.29x1038H combis9. If the accepted value for the heat of combustion for chicken fat is 30,038 kJ/mol calculate the percenterror.your answer - accepted answer|% Error-x 100accepted answer% Error =This experiment does not consider that all of the conditions are standard state conditions; therefore,you are calculating AHcomb not AH°comb.10. The "calorie" used to measure the caloric content of foods is actually a kilocalorie (kcal) or 4184 kJ.If the heat of combustion for sugar is 5639 kJ/mol, why are people who are on limited calorie dietsadvised to limit their fat intake?11. The food that we ingest is certainly not "combusted" in the same manner as is done in a bombcalorimeter.Why can we compare the heats of combustion of sugar or chicken fat measured in a bombcalorimeter with the caloric content of those foods?

Answer to sub-parts 9, 10 and 11 The answers to 6, 7 and 8 were found to be correct in accordance…

9. If the accepted value for the heat of combustion for chicken fat is 30,038 kJ/mol calculate the percent error. your answer - accepted answer|. % Error = x 100 accepted answer % Error = This experiment does not consider that all of the conditions are standard state conditions; therefore, you are calculating AHcomb not AH°comb. 10. The "calorie" used to measure the caloric content of foods is actually a kilocalorie (kcal) or 4184 kJ. If the heat of combustion for sugar is 5639 kJ/mol, why are people who are on limited calorie diets advised to limit their fat intake? 11. The food that we ingest is certainly not "combusted" in the same manner as is done in a bomb calorimeter. Why can we compare the heats of combustion of sugar or chicken fat measured in a bomb calorimeter with the caloric content of those foods?

9. If the accepted value for the heat of combustion for chicken fat is 30,038 kJ/mol calculate the percent error. your answer - accepted answer|. % Error = x 100 accepted answer % Error = This experiment does not consider that all of the conditions are standard state conditions; therefore, you are calculating AHcomb not AH°comb. 10. The "calorie" used to measure the caloric content of foods is actually a kilocalorie (kcal) or 4184 kJ. If the heat of combustion for sugar is 5639 kJ/mol, why are people who are on limited calorie diets advised to limit their fat intake? 11. The food that we ingest is certainly not "combusted" in the same manner as is done in a bomb calorimeter. Why can we compare the heats of combustion of sugar or chicken fat measured in a bomb calorimeter with the caloric content of those foods?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Propane reacts with oxygen gas to produce carbon dioxide and water as shown in the reaction below. How much energy in kJ will be released if 500 kg of propane is burned in the air? C3H8 + 50₂ 3CO₂ + 4H₂0 AH = -2221 kJ
|| Question 15 A calorimeter holds 25 g water at 25.0°C. A sample of hot iron is added to the water, and the final temperature of the water and iron is 30.0°C. What is the change in en- thalpy associated with the change in the water's temperature? Note: The specific heat of water is 4.18 g°c. Use the formula AH = - cm AT %3D Show your work. IUS
A chemist measures the energy change AH during the following reaction: Cl₂(g) + H₂(g) → 2 HC1 (g) AH=184. kJ Use the information to answer the following questions. endothermic. This reaction is... 0 exothermic. Suppose 28.0 g of Cl₂ react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. ☐kJ x10 X ?
A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q = specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the sblution increases to 30.0 °C At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, qp; that is, Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. ΔΗp Express the…
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
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A chemist carefully measures the amount of heat needed to raise the temperature of a 399.0 g sample of a pure substance from 4.1 °C to 19.7°C. The experiment shows that 865. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. -1 -1 J.g •K x10 Submit Assignme Continue 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibili I IMG-6111.jpg IMG-6110.jpg IMG-6109.jpg IMG-6108.jpg IMG-6107.jpg MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ # $ % & 2 3 4 5 6 7 8 9
they are the part of one question. kindly do all A,B,C
1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. = 7.52 g = 7.20 g Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.