The equilibrium concentrations in a gas mixture at a particular temperature are 0.13 M H2, 0.70 M I2, and 2.1 M HI. What equilibrium concentrations are obtained at the same temperature when 0.20 mol of HI is injected into an empty 500.0-mL container?

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In a closed system, this state can be described by the equilibrium constant (K), which relates the concentrations of the products and reactants at equilibrium. Understanding this concept is crucial for predicting how changes in concentration affect the system.

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how the addition of a substance, such as HI in this case, will shift the equilibrium position, affecting the concentrations of all species involved.

Concentration calculations involve determining the molarity (M) of a solution, which is defined as the number of moles of solute per liter of solution. In this scenario, after injecting HI into a 500.0-mL container, it is essential to calculate the new concentrations of H2, I2, and HI to analyze the system's response to the added reactant and establish the new equilibrium state.