9:06 AM Fri Aug 18← →3.4 Assignment - XContents [hide](Top)Material Safety Data SheetStructure and propertiesCited sources9:06 AM Fri Aug 18Thermodynamic propertiesVapor pressure of liquidSpectral dataReferences89:07 AM Fri Aug 18e of liquidContents [hide](Top)Material Safety Data SheetStructure and propertiesThermodynamic propertiesVapor pressure of liquidMelting point dataSpectral dataReferencesy Data Sheet9:07 AM Fri Aug 18W Methane (data pag Xata Sheeteouspertiespropertiesaqueousen.wikipedia.org/wiki/Methane_(data_page)liquid- at variousSiStd enthalpy changeof formation, AH liquidStandard molar entropy,SeliquidgasHeat capacity, CpStdchangeof formation, AH gasLogin iLearn BC Xvan der Waals' constants[10]T(°C)SesolidStandard molar entropy,SegasEnthalpy of combustion AH-891 kJ/mol[⁹]Heat capacity, Cp35.7 J/(mol K)[8]a = 228.29 L² kPa/mol²b= 0.04278 L/molsolidVapor pressure of liquid [edit]P(mm 1Hg)3.4 Assignment - X W Propane (data pag XHeat capacity, CpStd enthalpy changeof formation, AH liquid10gasStandard molar entropy,SºliquidHeat capacity, CpStd enthalpy changeof formation, AHStandard molar entropy,SoliquidHeat capacity, Cpgas3.4 Assignment - X W Ethanol (data page X? J/(mol K)Gas propertiesvan der Waals' constants[¹]en.wikipedia.org/wiki/Propane_(data_page)10-205.9 -195.5 -187.7 -181.4 -168.8 -161.5 -152.3 -138.3 -124.8 -108.5 -86.3Std enthalpy changeof formation, AH gasStandard molar entropy,SeHeat capacity, Cp? kJ/molLiquid properties? J/(mol K)I Login - iLearn BC Xvan der Waals' constants[²]-74.6 kJ/mol[8]40I Login - iLearn BC X186.3 J/(mol K)[8]en.wikipedia.org/wiki/Ethanol_(data_page)40Std enthalpy changeof formation, AH liquidEnthalpy of combustion, AH -1560.7 kJ/molHeat capacity, CpGas propertiesVapor pressure of liquid [edit]Pinmm 1Hg...Std enthalpy changeof formation, AH gasStandard molar entropy100UTIVLogin - iLearn BC X? J/(mol K)? kJ/mol126.7 J/(mol K)68.5 J/(mol K) at -179 °C-83.8 kJ/mol229.6 J/(mol K)52.49 J/(mol K) at 25 °Ca = 556.2 L² kPa/mol²b= 0.06380 L/mol100....400Gas propertiesLogin iLearn BC X98.36 J/(mol K)400 760-104.7 kJ/molEnthalpy of combustion, AH -2220.0 kJ/molHeat capacity, Cp73.60 J/(mol K)a = 877.88 L² kPa/mol²b = 0.08445 liter per mole....269.91 J/(mol K)760Login - iLearn BC XLiquid properties-277.38 kJ/molStandard molar entropy,So liquidEnthalpy of combustion, AH-1370.7 kJ/mol112.4 J/(mol K)Heat capacity, CpGas properties111.46 J/(mol K) [5]159.9 J/(mol K)006-235.3 kJ/mol1Login - iLearn BC X G Compare your calc x + 61520 3800LIZ15203800 7600Login - iLearn BC XDensity of liquid and gas [edit]Propane is highly temperature dependent. The density of liquid and gaseous propane are gimago7600B@@ 81%15200 30400 4560081%15200 30400 45600(a@ 81%G Compare your calc X +III@81%Login - iLearn BC X G Compare your calc x +=6III=þ6 4) Take the real AH values for the four compounds from the linked data sources and divideeach by the number of moles of O₂ that react per mole of fuel. (For example, 3.5 0₂'sreact with 1 ethane.) This will give you a AH per mole of oxygen for the reaction. What doesthis result say about the amount of energy that can be released from combustion reactions?

Given Compounds:Methane Ethane Propane Etanol To determine per mole oxygen of the reaction

Take the real AH values for the four compounds from the linked data sources and divide each by the number of moles of O₂ that react per mole of fuel. (For example, 3.5 0₂'s react with 1 ethane.) This will give you a AH per mole of oxygen for the reaction. What does this result say about the amount of energy that can be released from combustion reactions?

Take the real AH values for the four compounds from the linked data sources and divide each by the number of moles of O₂ that react per mole of fuel. (For example, 3.5 0₂'s react with 1 ethane.) This will give you a AH per mole of oxygen for the reaction. What does this result say about the amount of energy that can be released from combustion reactions?

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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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)
(Incorrect) Consider the following reaction: 2 PbS (s) + 3 02 (g) → 2 PbO (s) +2 SO₂ (g) AHxn=-827.4 kJ What mass of PbS has reacted if 765 kJ of heat is produced? You answered: 221. The correct answer is: 442.0g A
33 a b C d e Consider the hypothetical thermochemical equation 3A+B→2C for which AH = 61.5 kJ/mol. L L L L L If you have 5.30 moles of A, what quantity of heat, in kJ, would be absorbed? If the reaction absorbs 345 kJ of heat, What quantity in moles of C would be produced? What would AH, in kJ/mol, be for the reaction 2 C → 3 A + B? What would AH, in kJ/mol, be for the reaction 9A + 3 B →6 C? Which one of the following reactions would have an enthalpy change of -2xAH? Here, AH refers to the enthalpy change of the original reaction.
A gas expands and does work on the surroundings equal to 6.14 L atm. At the same time, it releases 97 J of heat to the surroundings. What is the change in energy in J of the gas?
please answer part B, D, E, and F.
Consider the following chemical reaction:C3H8(g) + H2(g) → C2H6(g) + CH4(g) ΔH° = ?Calculate the enthalpy change for the reaction above using Hess’s law.Thermochemical data:H2(g) + ½O2(g) → H2O(l) ΔH° = –285.8 kJΔH°combustion for CH4(g) ΔH° = –890.0 kJ/molCO2(g) → C(s, graphite) + O2(g) ΔH° = +393.5 kJΔH°combustion for C2H6(g) ΔH° = –1560.0 kJ/molΔH°f for C3H8(g) ΔH° = –103.8 kJ/mol
In a calorimeter, a 2.0 g sample of magnesium is burned to form MgO. In doing so, 25.5 kJ of energy are released. What is the Heat of Combustion in kJ/mol of magnesium? с 306.2 1.54 x 1025 0.0392 514 25.5
If 10.22 g of a hydrocarbon is combusted inside of a bomb calorimeter with a heat capacity of 722J/C and temperature is raised by 9.5 Chow much heat was lost by the reaction in its combustion?