Question

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

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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 ΔGorx. 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?

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Answer 1

1. T=273+25 =298

ΔGorx =∆Horx –T * ∆Sorx= -92380 – 298*(-98.4) =-63056.8

Since ΔGorx is negative, the reaction is spontaneous.

2. ln Kp= -(ΔGorx) /(R*T)=63056.8/(8.314*298) =24.45

Kp = 1.134*10¹¹

Since Kp>1 , the reaction will occur in the forward direction.

[Note: in this case Kp=K

K is the equilibrium ratio of products to reactants. The value for K is large (greater than one) when the products dominate the mixture and small (less than one) when the reactants dominate the mixture:

• K > 1: products are favored
• K = 1: neither reactants nor products are favored
• K < 1: reactants are favored

If the reaction favors the products, it will occur in the forward (left-to-right) direction. If K is very large, the reaction will occur mostly to completion, using up almost all the reactants. If the reaction favors the reactants, it will occur in the reverse (right-to-left) direction. If K is very small, the reaction will use up almost all the products and make them into reactants.]