combustion and enthalphy I.II.ObjectivesTable 1.●Data sheetSpecific Heat ofWater, J/g-°CMass ofAluminum, gMass of Water, gTemperaturechange ofWater, °CIII.Determine the change in enthalpy combustion of alcoholsthrough researchIV.InitialTemperatureFinalTemperatureComplete and Name the tableEthanol4.184 J/g °C14 g298.5 gTable 2. Temperature of water before and after alcohol combustion.Temperature ofEthanolPropanolWater, °CTable 3.Alcohols Mass of alcohol burnt, gethanol3.65 g3.18 gpropanolbutanol0.95 g31 °CConclusion54 °CResults and DiscussionPropanol4.184 J/g °C13 g302 g31 °CButanol4.184 J/g °C50.5 °C14.1 g298.6 gButanol31 °C50 °CList down more of common alcohol and name the tableMolar mass of alcohol, g/mol46.07 g/mol60.0952 g/mol74.121 g/molIn your own words, discuss the results from this lab activity.In your own words, what can you conclude about the activity

I. II. Objectives Table 1. ● Data sheet Specific Heat of Water, J/g-°C Mass of Aluminum, g Mass of Water, g Temperature change of Water, °C III. IV. Determine the change in enthalpy combustion of alcohols through research Initial Temperature Final Temperature Table 2. Temperature of water before and after alcohol combustion. Temperature of Ethanol Propanol Water, °C Complete and Name the table - Ethanol 4.184 J/g °C 14 g 298.5 g Table 3. Alcohols Mass of alcohol burnt, g ethanol 3.65 g 3.18 g propanol 0.95 g butanol 31 °C Conclusion 54 °C Results and Discussion Propanol 4.184 J/g °C 13 g 302 g 31 °C Butanol 4.184 J/g °C 14.1 g 298.6 g 50.5 °C Butanol 31 °C 50 °C List down more of common alcohol and name th Molar mass of alcohol, g/mol 46.07 g/mol 60.0952 g/mol 74.121 g/mol In your own words, discuss the results from this lab activity. In your own words, what can you conclude about the activity

I. II. Objectives Table 1. ● Data sheet Specific Heat of Water, J/g-°C Mass of Aluminum, g Mass of Water, g Temperature change of Water, °C III. IV. Determine the change in enthalpy combustion of alcohols through research Initial Temperature Final Temperature Table 2. Temperature of water before and after alcohol combustion. Temperature of Ethanol Propanol Water, °C Complete and Name the table - Ethanol 4.184 J/g °C 14 g 298.5 g Table 3. Alcohols Mass of alcohol burnt, g ethanol 3.65 g 3.18 g propanol 0.95 g butanol 31 °C Conclusion 54 °C Results and Discussion Propanol 4.184 J/g °C 13 g 302 g 31 °C Butanol 4.184 J/g °C 14.1 g 298.6 g 50.5 °C Butanol 31 °C 50 °C List down more of common alcohol and name th Molar mass of alcohol, g/mol 46.07 g/mol 60.0952 g/mol 74.121 g/mol In your own words, discuss the results from this lab activity. In your own words, what can you conclude about the activity

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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If 0.24 mols of substance B is able to produce 137J of heat. What is the change in reaction enthalpy in J associated with the following balanced reaction. (Hint: *pay attention the the coefficient for substances B *determine the sign for heat, is it + or -). Round and report your answer to an integer without decimal place including + or- - sign. Only enter numeric value, no unit. A+2B → AB2 + heat AHren =???
Suppose that the molar enthalpy of a reaction is -69.06 kJ/mol and 1.134 moles are reacted. How many kilojoules of heat are released by the reaction? Report your answer to three decimal places (ignore significant figures).
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This is a Biophysical Chemistry Question What is the difference between the heat capacity of a substance and the heat capacity change of a reaction? Why is it important to know whether a reaction has an overall heat capacity change?
A east.cengagenow.com/ilrn/takeAssignment/takeCXPCompliantActivity.do?locator=Dassignment-take References Use the References to access Important values If needed for this question. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.5021 g sample of heptadecanoic acid (C,,H,0,) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.246x10 g of water. During the combustion the temperature increases from 21.91 to 25.07 °C. The heat capacity of water is 4.184 Jg1°C1. tin The heat capacity of the calorimeter was determined in a previous experiment to be 822.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. Cmbe te car C,,H3402(s) + (49/2) O2(g) → 17 H2O(1) + 17 CO2(g) + Energy kJ/mol Molar Heat of Combustion = Save and Exit Cengage Learning | Cengage…
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?
The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…
What will happen to the enthalpy of combustion if the bomb calorimeter contains less than 2.0 L of water before the combustion?
How much heat is released when 75g of octane is burned completely if the enthalpy of combustion is -5,500KJ/mol octane?