The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4 NH 3 ( g ) + 5 O 2 → 4 NO ( g ) + 6 H 2 O ( g ) 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) 3 NO 2 ( g ) + H 2 O ( l ) → 2 HNO 3 ( a q ) + NO ( g ) a. Use the values of Δ H f ° in Appendix 4 to calculate the value of ∆Hº for each of the preceding reactions. b. Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations. (Water is also a product.) Is the overall reaction exothermic or endothermic?
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4 NH 3 ( g ) + 5 O 2 → 4 NO ( g ) + 6 H 2 O ( g ) 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) 3 NO 2 ( g ) + H 2 O ( l ) → 2 HNO 3 ( a q ) + NO ( g ) a. Use the values of Δ H f ° in Appendix 4 to calculate the value of ∆Hº for each of the preceding reactions. b. Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations. (Water is also a product.) Is the overall reaction exothermic or endothermic?
Solution Summary: The author explains Hess's Law: Standard enthalpy of formation. The quantity of reactants and products is directly proportional to the magnitude of H in a reaction.
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps:
4
NH
3
(
g
)
+
5
O
2
→
4
NO
(
g
)
+
6
H
2
O
(
g
)
2
NO
(
g
)
+
O
2
(
g
)
→
2
NO
2
(
g
)
3
NO
2
(
g
)
+
H
2
O
(
l
)
→
2
HNO
3
(
a
q
)
+
NO
(
g
)
a. Use the values of
Δ
H
f
°
in Appendix 4 to calculate the value of ∆Hº for each of the preceding reactions.
b. Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations. (Water is also a product.) Is the overall reaction exothermic or endothermic?
Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NO2 (g) = N2O4(g)
AGº = -5.4 kJ
Now suppose a reaction vessel is filled with 4.53 atm of dinitrogen tetroxide (N2O4) at 279. °C. Answer the following questions about this system:
Under these conditions, will the pressure of N2O4 tend to rise or fall?
Is it possible to reverse this tendency by adding NO2?
In other words, if you said the pressure of N2O4 will tend to rise, can that
be changed to a tendency to fall by adding NO2? Similarly, if you said the
pressure of N2O4 will tend to fall, can that be changed to a tendency to
'2'
rise by adding NO2?
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO 2 needed to reverse it.
Round your answer to 2 significant digits.
00
rise
☐ x10
fall
yes
no
☐ atm
G
Ar
1
Why do we analyse salt?
Curved arrows are used to illustrate the flow of electrons. Using
the provided starting and product structures, draw the curved
electron-pushing arrows for the following reaction or
mechanistic step(s).
Be sure to account for all bond-breaking and bond-making
steps.
H
H
CH3OH, H+
H
Select to Add Arrows
H°
0:0
'H
+
Q
HH
■ Select to Add Arrows
CH3OH,
H*
H.
H
CH3OH, H+
HH
■ Select to Add Arrows i
Please select a drawing or reagent from the question area
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