Part ACalculate the enthalpy of the reaction2NO(g) + O2(g)→2NO2(g)given the following reactions and enthalpies of formation:1. N2(g)+ O2(g)→NO2(g),2. N2 (g) + 302(g)→NO(g), AH3 = 90.2 kJAH = 33.2 kJExpress your answer with the appropriate units.• View Available Hint(s)– 144kJΔΗ' -SubmitPrevious AnswersX Incorrect; Try Again; 3 attempts remainingPart BCalculate the enthalpy of the reaction4B(s) + 302(g)→2B2O3(s)given the following pertinent information:1. B203(s) + 3H20(g)→302(g) +B2H6(g),2. 2B(s) + 3H2(g)→B2H6(g),3. H2(g) + O2(g)→H2O(1),4. H20(1)→H20(g),AH{AHAH:=-285 kJAHB = +44 kJ+2035 kJ= +36 kJExpress your answer with the appropriate units.• View Available Hint(s)НАΔΗValueUnitsSubmit

Determination of enthalpy of the reaction: Given equation:

Answered: Part A Calculate the enthalpy of the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.41QE

See similar textbooks

Similar questions

9.73 Without looking up any numerical data or doing calculations, predict whether the enthalpy change for each of the following reactions should he positive, negative, or zero. (a) H2O(l)H2O(s) (b) N2(g)2N(g) (c) CH4(g)+2O2(g)CO2(g)+2H2O(l) (d) CO2(s)CO2(g)
Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the balanced equation for the combustion of ethanol to CO2(g) and H2O(g), and, using the data in Appendix G, calculate the enthalpy of combustion of 1 mole of ethanol. (b) The density of ethanol is 0.7893 g/mL. Calculate the enthalpy of combustion of exactly 1 L of ethanol. (c) Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n—octane, C8H18(Hf=208.4kJ/mol;density=0.7025g/mL).
Chloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) 3 HCl(g) + CHCl3(g) Calculate rH, the enthalpy change for this reaction, using the enthalpies of formation of CO2(g), H2O(), CHCI3(g) (fH = 103.1 kJ/mol), and the enthalpy changes for the following reactions: CH4(g) + 2 O2(g) 2 H2O() + CO2(g) rH = 890.4 kJ/mol-rxn 2 HCl(g) H2(g) + Cl2(g) rH = +184.6 kJ/mol-rans
A 10.00-g sample of acetic acid, HC2H3O2, was burned in a bomb calorimeter in an excess of oxygen. HC2H3O2(l)+2O2(g)2CO2(g)+2H2O(l) The temperature of the calorimeter rose from 25.00C to 35.84C. If the heat capacity of the calorimeter and its contents is 13.43 kJ/C, what is the enthalpy change for the reaction?
The head of a strike anywhere match contains tetraphosphorus trisulfide, P4S3. In an experiment, a student burned this compound in an excess of oxygen and found that it evolved 3651 kJ of heat per mole of P4S3 at a constant pressure of 1 atm. She wrote the following thermochemical equation: P4S3(s)+8O2(g)P4O10(s)+3SO2(g);H=3651kJ Calculate the standard enthalpy of formation of P4S3, using this students result and the following standard enthalpies of formation: P4O10(s), 3009.9 kJ/mol; SO2(g), 296.8 kJ/mol. How does this value compare with the value given in Appendix C?
Calcium oxide, CaO, is prepared by heating calcium carbonate (from limestone and seashells). CaCO3(s)CaO(s)+CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation. The Hf of CaO(s) is 635 kJ/mol. Other values are given in Table 6.2.
Sodium carbonate, Na2CO3, is used to manufacture glass. It is obtained from sodium hydrogen carbonate, NaHCO3, by heating. 2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation (Table 6.2).
Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide. 2H2S(g)+3O2(g)2SO2(g)+2H2O(g);H=1036kJ Calculate the enthalpy change to burn 27.4 g of hydrogen sulfide.
Give the definition of the standard enthalpy of formation for a substance. Write separate reactions for the formation of NaCl, H2O , C6H12O6, and PbSO4 that have H values equal to Hf for each compound.
Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2H4O, by the reaction C2H4O(g)+H2O(l)HOCH2CH2OH(l) Use Hesss law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C2H4O(g)+5O2(g)4CO2(g)+4H2O(l);H=2612.2kJHOCH2CH2OH(l)+52O2(g)2CO2(g)+3H2O(l);H=1189.8kJ
The combustion of ethane, C2H6, has an enthalpy change of 2857.3 kJ for the reaction as written below. Calculate H for the combustion of 15.0 g of C2H6. 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) rH=2857.3kJ/mol-rxn
Which of the following substances have an enthalpy of formation equal to zero? a. Cl2(g) b. H2(g) c. N2(l) d. Cl(g)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS