Given the following equations and AH° values given below, determine the heat of reaction at 298K for the following reaction: 2 N2(g) + 5O2lg) → 2 N2O5(g)14.2 H2(g) + O2(g) –2 H20(1)AH° = -571.6 kJN2Os(g) + H20(1)→ 2 HNO3(1)AH° = -73.7 kJN2(g) +3 O2(g) + H2(g)2 HNO3(1)AH° = -348.2 kJ

Given, a) 2H2(g) + O2(g) ➝ 2H2O(l) ∆H° = -571.6 kJ b) N2O5(g) + H2O(l) ➝ 2HNO3(l) ∆H° = -73.7 kJ c)…

14. Given the following equations and AH° values given below, determine the heat of reaction at 298 K for the following reaction: 2 N2(g) + 5 02(g) → 2 N2Os(g) 2 H2(g) + O2(g)→ 2 H2O(I) AH° = -571.6 kJ N2O5(g) + H20(1)→2 HNO3(1) AH° = -73.7 kJ N2(g) + 3 O2(g) + H2(g)2 HNO3(1) AH° = -348.2 kJ

14. Given the following equations and AH° values given below, determine the heat of reaction at 298 K for the following reaction: 2 N2(g) + 5 02(g) → 2 N2Os(g) 2 H2(g) + O2(g)→ 2 H2O(I) AH° = -571.6 kJ N2O5(g) + H20(1)→2 HNO3(1) AH° = -73.7 kJ N2(g) + 3 O2(g) + H2(g)2 HNO3(1) AH° = -348.2 kJ

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 30P

See similar textbooks

Similar questions

Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
The octane number of gasoline is based on a comparison of the gasolines behavior with that of 2,2,4-trimethylpentane, C8H18(), which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is 5456.6 kJ/mol. (a) Write the thermochemical equation for the combustion of 2,2,4-trimethylpentane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of 2,2,4-trimethylpentane.
The standard enthalpy of formation of H2O(l) at 298 K is 285.8 kJ/mol. Calculate the change in internal energy for the following process at 298 K and 1 atm: H2O(l)H2(g)+12O2(g)E=? (Hint: Using the ideal gas equation, derive an expression for work in terms of n, R, and T.)
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Calculate rS for each substance when the quantity of thermal energy indicated is transferred reversibly to the system at the temperature specified. Assume that youhave enough of each substance so that its temperatureremains constant as the thermal energy is transferred. (a) H2(g), 0.775 kJ/mol, 295 K (b) KCl(s), 500. kJ/mol, 500. K (c) N2(g), 2.45 kJ/mol, 1000. K
Explain inyour own words why work done by the system is defined as the negative of pV, not positive pV.
Calculatethe work performed by a person whoexertsa force of 30 NN = newtonstomove abox 30metersif the force were a exactly parallel to the directionofmovement, and b45to thedirection of movement. Do the relative magnitudesmakesense?