Consider the reaction 4 hcl(g) + o2(g) =2 h2o(g) + 2 cl2(g) using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15k.

delta g (kj/mol)

hcl=-95.3

o2=0

h2o=-228.6

cl2=0

The equilibrium constant for this reaction at 298.15 K is .

Explanation:

The equation used to calculate Gibbs free change is of a reaction is:  

The equation for the enthalpy change of the above reaction is:

We are given:

(pure element)

Putting values in above equation, we get:

To calculate the (at 25°C) for given value of Gibbs free energy, we use the relation:

where,

= Gibbs free energy = -76 kJ/mol = -76000 J/mol  

(Conversion factor: 1kJ = 1000J)

R = Gas constant =

T = temperature = 298.15 K[/tex]

= equilibrium constant at 25°C = ?

The equilibrium constant for this reaction at 298.15 K is .

the product of the pressure and volume is also constant

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