Complete the table relating the values of Īšŗā and š¾ .
Īšŗā K
<0
=0
>0
K can be =1, <1, or >1
Īšŗā K
<0 ; K > 1
=0 ; K = 1
>0 ; K < 1
ĪGĀ° K
<0 >1
=0 =1
>0 <1
Complete table relating the values of Īšŗā and š¾:
Īšŗā K
<0 K > 1
=0 K = 1
>0 K < 1
To complete the table relating the values of Īšŗā and š¾, we need to understand their relationship.
Īšŗā represents the change in Gibbs free energy, which is a measure of the thermodynamic potential for a chemical reaction. It determines the direction in which a reaction will proceed. If Īšŗā is negative, it means the reaction is thermodynamically favorable and will tend to proceed in the forward direction. If Īšŗā is positive, it means the reaction is thermodynamically unfavorable and will tend to proceed in the reverse direction. If Īšŗā is zero, it means the reaction is at equilibrium, with equal amounts of reactants and products.
On the other hand, š¾ represents the equilibrium constant, which quantifies the extent to which a reaction proceeds. It is defined as the ratio of the concentrations (or partial pressures) of the products to the concentrations (or partial pressures) of the reactants, each raised to the power of their stoichiometric coefficients.
Now, let's complete the table:
If Īšŗā is negative, indicating a thermodynamically favorable reaction, š¾ will be greater than 1. This means the concentrations (or partial pressures) of the products will be greater than the concentrations (or partial pressures) of the reactants at equilibrium.
If Īšŗā is zero, the reaction is at equilibrium. In this case, š¾ will be equal to 1, indicating that the concentrations (or partial pressures) of the reactants and products are equal.
If Īšŗā is positive, indicating a thermodynamically unfavorable reaction, š¾ will be less than 1. This means the concentrations (or partial pressures) of the reactants will be greater than the concentrations (or partial pressures) of the products at equilibrium.
Therefore, the completed table would look as follows:
Īšŗā K
<0 >1
=0 =1
>0 <1