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 .

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i  

b.false that your answer