Answer to Question #163088 in Organic Chemistry for stephen

Question

Calculate the enthalpy change for the production of one mole of dinitrogen

pentoxide gas from nitrogen gas and oxygen gas. Use the thermochemical equations

a., b., and c. Show all your work. Beside each equation write the changes you are

making to each equation, re-write the equations according to your changes. Your

answer must include a balanced thermochemical equation. Include a potential energy

diagram for your target equation. (5 marks)

a. 2H2(g) + O2(g) ® 2H2O(l) DH° = -572.0 kJ

b. . N2O5(g) + . H2O(l) ® HNO3(l) DH° = -38.5 kJ

c. !

" N2(g) + #

" O2(g) + !

" H2(g) ® HNO3(l) DH° = -174.0 kJ

Answer 1

N_2(g) + 3O_2(g) + H_2(g) = 2HNO_3(l) DH = -174.0 kJ / -H_2(g), -0.5O_2(g), +H₂O_(l), +572 kJ/2

N_2(g) + 2.5O_2(g) + H₂O_(l) = 2HNO_3(l) DH = 112 kJ / -2HNO_3(l), -H₂O_(l), +N₂O_5(g), +38.5 kJ

N_2(g) + 2.5O_2(g) = N₂O_5(g) DH = 150.5 kJ