75.4k views
2 votes
When K (>/=/<) 1, ΔG° is 0 and the reaction is at equilibrium under standard conditions. a) 0

b) negative
c) positive
d) undefined

User Peter Reid
by
8.0k points

1 Answer

1 vote

Final answer:

When K = 1, ΔG° is 0, meaning that the reaction is at equilibrium under standard conditions and neither reactants nor products are favored.

Step-by-step explanation:

When K = 1, ΔG° is 0 and the reaction is at equilibrium under standard conditions. At this point, the system has reached a state where neither reactants nor products are favored, meaning that the forward and reverse reactions occur at the same rate, leading to a dynamic balance. The equilibrium constant K indicates the ratio of product concentrations to reactant concentrations at equilibrium, and ΔG° represents the standard free energy change associated with a chemical reaction.


If ΔG° < 0, the equilibrium constant K will be greater than 1, indicating a spontaneous reaction in the forward direction where products are favored. Conversely, if ΔG° > 0, K will be less than 1, and the reverse reaction is spontaneous, favoring reactants. Therefore, when K equals 1, ΔG° equals to 0, indicating that the system is at equilibrium and no net reaction is occurring.

User Patricio Vargas
by
7.0k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.