Please answer and show all work and units. Will rate ASAP. ---------------------

Question

Please answer and show all work and units. Will rate ASAP.
-------------------------------------------------------------------------------------------------------
Consider the reaction shown below taking place at 25oC
N2(g) + 3 H2 (g) 2 NH3 (g)
For this reaction it has been found that Horx = - 92.38 kJ and Sorx= - 98.4 J/K
A) Calculate the value of Gorx. Is this reaction spontaneous? Why or why not?
B) Calculate the value of the equilibrium constant, Kp, for this reaction. In which direction is the equilibrium displaced?
------------------------------------------------------------------------------------------------------- Please answer and show all work and units. Will rate ASAP.
-------------------------------------------------------------------------------------------------------
Consider the reaction shown below taking place at 25oC
N2(g) + 3 H2 (g) 2 NH3 (g)
For this reaction it has been found that Horx = - 92.38 kJ and Sorx= - 98.4 J/K
A) Calculate the value of Gorx. Is this reaction spontaneous? Why or why not?
B) Calculate the value of the equilibrium constant, Kp, for this reaction. In which direction is the equilibrium displaced?
------------------------------------------------------------------------------------------------------- Please answer and show all work and units. Will rate ASAP.
-------------------------------------------------------------------------------------------------------
Consider the reaction shown below taking place at 25oC
N2(g) + 3 H2 (g) 2 NH3 (g)
For this reaction it has been found that Horx = - 92.38 kJ and Sorx= - 98.4 J/K
A) Calculate the value of Gorx. Is this reaction spontaneous? Why or why not?
B) Calculate the value of the equilibrium constant, Kp, for this reaction. In which direction is the equilibrium displaced?
-------------------------------------------------------------------------------------------------------

Explanation / Answer

For the given reaction,

T = 25 + 273 = 298 K

A) dGorxn = dHorxn - TdSorxn

                  = -92.38 - 298 x -0.0984        

                  = -63.0568 kJ/mol

The reaction is spontaneous as the net change in free energy of reaction is -ve.

B) Using,

dGo = -RTlnKp

-63056.8 = -8.314 x 298 lnKp

Kp = 1.13 x 10^11

Kp is very high, the direction of equilibrium displacement would be to the right, towards product formation.

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.