For the reaction NO(g) + NO₂(g) the following questions. Substance NO(g) NO₂(g) N₂O(g) N₂O3 (9) N₂O4 (9) N₂O5 (9) N₂O5 (8) AHºt So (kJ.mol-¹) (J.mol-¹.K-¹) 90.25 210.7 33.2 kJ 82.05 83.72 9.16 11 N₂O3(g), use thermodynamic data from the following table to calculate AH and AS°. Then use those values to answer -43.1 240.0 219.7 321.28 304.2 356 178 (a) Is this reaction spontaneous at 25°C? Explain your answer. The calculated AH and AS values result in a AG (in kJ) of (b) How will the spontaneity of the reaction change as the temperature increases? As the temperature increases, the TAS term of the Gibbs free energy equation will become more indicating a reaction. (c) To show that your prediction is accurate, calculate AG (in kJ) at 71°C. (Assume that both enthalpy and entropy are independent of temperature.) kJ at 25° C. Since AG is this reaction is and the value for AG
For the reaction NO(g) + NO₂(g) the following questions. Substance NO(g) NO₂(g) N₂O(g) N₂O3 (9) N₂O4 (9) N₂O5 (9) N₂O5 (8) AHºt So (kJ.mol-¹) (J.mol-¹.K-¹) 90.25 210.7 33.2 kJ 82.05 83.72 9.16 11 N₂O3(g), use thermodynamic data from the following table to calculate AH and AS°. Then use those values to answer -43.1 240.0 219.7 321.28 304.2 356 178 (a) Is this reaction spontaneous at 25°C? Explain your answer. The calculated AH and AS values result in a AG (in kJ) of (b) How will the spontaneity of the reaction change as the temperature increases? As the temperature increases, the TAS term of the Gibbs free energy equation will become more indicating a reaction. (c) To show that your prediction is accurate, calculate AG (in kJ) at 71°C. (Assume that both enthalpy and entropy are independent of temperature.) kJ at 25° C. Since AG is this reaction is and the value for AG
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:For the reaction NO(g) + NO₂(g) → N₂O3 (g), use thermodynamic data from the following table to calculate AH and AS. Then use those values to answer
the following questions.
Substance
NO(g)
NO₂(g)
N₂O(g)
N2O3 (9)
N₂O4 (9)
N₂O5 (9)
N₂O5 (s)
AH° f
(kJ. mol-¹) (J.
90.25
33.2
kJ
82.05
83.72
9.16
11
-43.1
Sr
J. mol-¹. K-
210.7
240.0
219.7
321.28
304.2
356
178
(a) Is this reaction spontaneous at 25°C? Explain your answer.
The calculated AH and AS values result in a AG (in kJ) of
(b) How will the spontaneity of the reaction change as the temperature increases?
As the temperature increases, the TAS term of the Gibbs free energy equation will become more
indicating a
reaction.
(c) To show that your prediction is accurate, calculate AG (in kJ) at 71°C. (Assume that both enthalpy and entropy are independent of temperature.)
kJ at 25°C. Since AG is
this reaction is
and the value for AG
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Step 1: Enthalpy, entropy, and Gibbs free energy
VIEWStep 2: Determination of enthalpy of the reaction
VIEWStep 3: Determination of entropy of the reaction
VIEWStep 4: Gibbs free energy at 25oC
VIEWStep 5: Effect of increase in temperature on Gibbs free energy
VIEWStep 6: Gibbs free energy at 71oC
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