Answer : K > 1is the true statement about the equilibrium constant for a reaction if [tex]\Delta G^o[/tex] for the reaction is negative.
Explanation :
The relation between the equilibrium constant and standard Gibbs, free energy is:
[tex]\Delta G^o=-RT\times \ln K[/tex]
where,
[tex]\Delta G^o[/tex] = standard Gibbs, free energy
R = gas constant
T = temperature
K = equilibrium constant
From the above relation we conclude that,
When K > 1 then the value of [tex]\Delta G^o[/tex] is negative.
When K < 1 then the value of [tex]\Delta G^o[/tex] is positive.
When K = 1 then the value of [tex]\Delta G^o[/tex] is zero.
When K = 0 then the value of [tex]\Delta G^o[/tex] is undefined.
Hence, K > 1is the true statement about the equilibrium constant for a reaction if [tex]\Delta G^o[/tex] for the reaction is negative.
The statement that is true if the reaction is negative is K > 1.
Equilibrium constant portrays the relationship between the products and reactants when a chemical reaction reaches equilibrium.
In a chemical reaction;
∆G° = standard Gibbs, free energy
R = gas constant
T = temperature
K = equilibrium constant
It can be said that;
Therefore, the statement that is true if the reaction is negative is K > 1.
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