E Give Up?= 21 of 28 QuestionsO Assignment Score:O Hint84.7%Check AnswerResourcesU 13 queaLIUITυυνο1 of o AttemptsCorrect< Question 21 of 28O 14 QuestionCalculate the heat energy released when 15.9 g of liquid100%Constants for mercury at 1 atm1 of o Attemptsmercury at 25.00 °C is converted to solid mercury at itsCorrectheat capacity of Hg(1)28.0 J/(mol-K)melting point.melting point234.32 KO 15 Question95%enthalpy of fusion2.29 kJ/mol2 of oo AttemptsCorrectO 16 Question100%1 of oo AttemptsCorrectkJqp =O 17 Question100%1 of o AttemptsCorrect18 QuestionO of oo Attempts0%O 19 Question100%1 of o AttemptsCorrect20 Question0%O of oo Attempts21 QuestionO of oo Attempts0%22 Question0%O of oo AttemptsO 23 Question1 of o Attempts100%CorrectO 24 Question100%1 of oo AttemptsCorrectQuestion Source: MRG - General Chemistry| Publisher: University Science Books

Answered: E Give Up? = 21 of 28 Questions O…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 81AP

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On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
You are attending summer school and living in a very old dormitory. The day is oppressively hot. there is no air conditioner, and you cant open the windows of your room. There is a refrigerator in the room, however. In a stroke of genius, you open the door of the refrigerator, and cool air cascades out. The relief does not last long, though. Soon the refrigerator motor and condenser begin to run, and not long thereafter the room is hotter than it was before. Why did the room warm up?
Liquid hydrogen fluoride, liquid water,and liquid ammonia all have relatively high specific heats for suchsmall molecules. Speculate asto whythis might be so.
Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?
How much energy is removed when 433 g of steam (MW = 18.02 g/mol) is cooled to 70.0 °C? ΔHfusion = 6.01 kJ/mol, heat capacity = 75.3 J/(mol °C), and ΔHVAP = 40.6 kJ/mol.
The standard enthalpies of formation of gaseous propyne1C3H42, propylene 1C3H62, and propane 1C3H82 are+185.4, +20.4, and -103.8 kJ>mol, respectively. (a) Calculatethe heat evolved per mole on combustion of each substance toyield CO21g2 and H2O1g2. (b) Calculate the heat evolved oncombustion of 1 kg of each substance. (c) Which is the mostefficient fuel in terms of heat evolved per unit mass?
Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 523.70 g sample of acetone gas has a temperature of 56.0°C. How much heat is involved in converting it to a solid that has a temperature of -94.0°C? (Answer in Joules)
Calculate the wirk done in Joules when 3 moles of water vaporize at 1.0 atm and 100ºC. Assmune the colume of liquid water is negligible compared with that of steam at 100ºC, and ideal gas behavoir. R= 0.0821 Latm/molK.
Dry nitrogen gas (100.0 L) was bubbled through liquid ethanol, C2H5OH, at a given temperature and the evaporated ethanol condensed; its mass was then measured. Using the data below, calculate the heat of vaporization (kJ/mol) of ethanol?
How much heat must be removed from a 90.5 g sample of benzene (M = 78.11 g mol-1) to cool the sample from 305 K to 215 K? The following physical data may be useful.ΔfusH = 9.8 kJ mol-1ΔvapH = 30.8 kJ mol-1Cs(l) = 1.73 J g-1 K-1Cs(s) = 1.51 J g-1 K-1Cs(g) = 82.4 J g-1 K-1 Tm = 279.0 KTb = 353.3 K Note: The word 'removed' in the question already accounts for the negative sign involved in the heat transfer. Express your answer to three significant figures.
(a) How much heat is released when 25.0 g of methaneburns in excess O₂ to form gaseous CO₂ and H₂O?(b) Calculate the temperature of the product mixture if themethane and air are both at an initial temperature of 0.0C.Assume a stoichiometric ratio of methane to oxygen from theair, with air being 21% O₂ by volume (c of CO₂=57.2 J/molK;c of H₂O(g)= 36.0 J/molK; c of N=230.5 J/molK).

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