1.. This question is given in the photo2..The Haber process is used to produce ammonia for fertilizers:N2(g)+3H2(g)→2NH3(g) The reaction is performed at 300 Kand 500 Kand found to have equilibrium constants of 3.9×105and 1.2×10−1, respectively. Calculate ΔHand ΔSfor the reaction. 4. Using the supplied data, calculate the equilibrium constant Kp for the following reaction at 25 °C:2NO2(g) + H₂O(1) → 2HNO3(aq) + NO(g)51.3 -237.1-110.9 87.6AG°f(kJ/mol)5. The Haber process is used to produce ammonia for fertilizers: N₂(g) + 3H₂(g) → 2NH3(g). The reaction isperformed at 300K and 500K and found to have equilibrium constants of 3.9x105 and 1.2x10-¹, respectively.Calculate AH and AS for the reaction.

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Answered: .. This question is given in the photo…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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

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

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 16PS: Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2...

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1.. This question is given in the photo

2..The Haber process is used to produce ammonia for fertilizers:

N₂(g)+3H₂(g)→2NH₃(g)

The reaction is performed at 300 Kand 500 Kand found to have equilibrium constants of 3.9×105and 1.2×10−1, respectively. Calculate ΔHand ΔSfor the reaction.

4. Using the supplied data, calculate the equilibrium constant Kp for the following reaction at 25 °C:
2NO2(g) + H₂O(1) → 2HNO3(aq) + NO(g)
51.3 -237.1
-110.9 87.6
AG°f(kJ/mol)
5. The Haber process is used to produce ammonia for fertilizers: N₂(g) + 3H₂(g) → 2NH3(g). The reaction is
performed at 300K and 500K and found to have equilibrium constants of 3.9x105 and 1.2x10-¹, respectively.
Calculate AH and AS for the reaction.

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