For a reaction at standard conditions, if ΔG° is negative, what can be said abou
Practice Questions
Q1
For a reaction at standard conditions, if ΔG° is negative, what can be said about the equilibrium constant (K)?
K < 1
K = 1
K > 1
K is undefined
Questions & Step-by-Step Solutions
For a reaction at standard conditions, if ΔG° is negative, what can be said about the equilibrium constant (K)?
Step 1: Understand what ΔG° means. ΔG° is the change in free energy for a reaction under standard conditions.
Step 2: Know that if ΔG° is negative, it means the reaction is spontaneous and can proceed in the forward direction.
Step 3: Learn about the equilibrium constant (K). K tells us the ratio of products to reactants at equilibrium.
Step 4: Remember that a K value greater than 1 means there are more products than reactants at equilibrium.
Step 5: Conclude that if ΔG° is negative, it indicates that the reaction favors the formation of products, which means K is greater than 1.
Gibbs Free Energy and Equilibrium Constant – The relationship between Gibbs free energy change (ΔG°) and the equilibrium constant (K) is given by the equation ΔG° = -RT ln(K), indicating that a negative ΔG° corresponds to a K value greater than 1, suggesting that products are favored at equilibrium.
