When adjusted for any changes in δh and δs with temperature, the standard free energy change δg∘t at 2400 k is equal to 1.22*105j/mol. calculate the equilibrium constant at 2400 k.?

Question

Chemistry

Marques Hensley

11 August, 04:49

When adjusted for any changes in δh and δs with temperature, the standard free energy change δg∘t at 2400 k is equal to 1.22*105j/mol. calculate the equilibrium constant at 2400 k.?

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Raymond Frost · Answer 1

When adjusted for any changes in δh and δs with temperature, the standard free energy change δg∘t at 2400 k is equal to 1.22*105j/mol, then the equilibrium constant at 2400 k is 2.21*10-3. The answer to the statement is 2.21*10-3.

Grace Tanner · Answer 2

The equilibrium constant of a reaction is related the Gibbs free energy in a natural logarithm relationship. It is expressed as:

G = - RT ln K

where R is 8.314 and T is the temperature. From this, we can easily calculate for the change in the equilibrium constant at different temperature.

1.22*105 = - 8.314 (2400) ln K

K = 2.21x10^-3