dont provide handwriting soluton..... 3. One method that can produce hydrogen isocyanide is the following reaction:HHH+= ?:CEN H+3 H HAUrxnUse the average bond energy data below to estimate the value of AU in units of kJ.a. -575 kJb. -220 kJAverage bond energyBondH-H435 kJ/molc. +245 kJC-H415 kJ/mold. +490 kJe. +615 kJN-H390 kJ/molC-N305 kJ/molC=N615 kJ/molC=N890 kJ/molh

Let's break down the process step by step: 1. Understanding Bond Energy: Bond energy refers to the…

Answered: 3. One method that can produce hydrogen…

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 49P

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Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of SO2 must be evaporated to remove as much heat as evaporation of 1.00 kg of CC12F2 (enthalpy of vaporization is 17.4 kJ/mol)? The vaporization reactions for SO2 and are SO2(l)SO2(g) and CCl2F(l)CCl2F2(g), respectively.
At constant pressure and 25^C, What is delta H for the following reaction. 2C2H6(g) + 7O2(g) = 4CO2(g) + H2O(l) if the complete consumption of 38.2 g of C2H6 libraties 1981 KJ of heat energy?
Standard Enthalpy of Formations in kJ/mol at 298.15 K ΔHof ΔHof AlCl3(s) -704.2.0 Al2O3(s) -1676 H2O(l) -285.8 H2O(g) -241.8 NH4ClO3(s) -265.2 N2O(g) 81.6 Use data above to calculate the enthalpy change for the reaction: 6Al(s) + 6NH4ClO3(s) => 2Al2O3(s) + 2AlCl3(s) + 3 N2(g) + 12H2O(g) ΔH = ?
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?
How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 k to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful.DHvap = 33.9 kJ/molDHfus = 9.8 kJ/molCliq = 1.73 J/g°CCgas = 1.06 J/g°CCsol = 1.51 J/g°CTmelting = 279.0 KTboiling = 353.0 K
Calculate the enthalpy change for the reaction C(s) + 2H2 (g)--->CH4(g) from the following data. C(s) + O2 (g) ---> CO2(g). ΔH = – 393.5 kJ/mol H2(g) + 0.5 O2 (g) ---> H2O(l). ΔH = – 285.8 kJ/mol CH4(g) + 2 O2 (g)---> CO2(g) + 2 H2O(l). ΔH = – 890.2 kJ/mol
How much energy must be removed from a 125 g sample of benzene (molar mass = 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful. ΔHvap = 33.9 kJ/mol ΔHfus = 9.8 kJ/mol Cliq = 1.73 J/g°C Cgas = 1.06 J/g°C Csol = 1.51 J/g°C Melting pt = 279.0 K Boiling pt = 353.0 K
(a) In polyvinyl chloride shown in Table 12.6, whichbonds have the lowest average bond enthalpy? (b) When subjected to high pressure and heated, polyvinylchloride converts to diamond. During this transformationwhich bonds are most likely to break first? (c)Employing the values of average bond enthalpy in Table8.3, estimate the overall enthalpy change for convertingPVC to diamond.
Is ther an error in the solution that ∆Grxn=−9.33 kJ/mol=9330 J/mol was not kept negative when converted tfrom kJ to J? Can steps 3-5 be checked for accuracy ?
a) Calculate the standard enthalpy of formation of NaHCO3(s) given the following information:Δf?°[CO2(g)] = −393.41 kJ mol-1; Δf?° [ NaOH(s) ] = −425.61 kJ mol-1; Δrxn?° [NaOH(s) + CO2(g)⟶NaHCO3(s) ] = −127.5 kJ mol-1 b) Construct a diagram depicting Δrxn?° of the above reaction and the standardenthalpies of formation of the associated products and reactants.
Calculate the standard enthalpy change for the following reaction:2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Given: CH3OH(l) ?Hf0 = - 238.7 kJ/mol O2(g) ?Hf0 = 0 kJ/mol CO2(g) ?Hf0 = - 393.5 kJ/mol H2O(l) ?Hf0 = - 285.8 kJ/mol
At constant pressure and 25℃, what is ∆H° for the following reaction 2C2H6 (g)+7O2 (g)→4CO2 (g)+H2O(l) If the complete consumption of 38.2g of C2H6 liberates 1981 kJ of heat energy?

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