Consider the following statements regarding chemical equilibrium and Le Chatelier's principle: 1. If an exothermic equilibrium reaction is subjected to an increase in temperature, the equilibrium shifts in the backward direction to absorb the added heat. 2. An increase in pressure on a gaseous equilibrium mixture favors the direction that produces a smaller number of moles of gas. Which of the statements given above is/are correct?

💡 Solution & Explanation

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing conditions, the position of equilibrium shifts to counteract the change. An exothermic reaction releases heat, so raising the temperature favors the endothermic reverse reaction. Increasing pressure forces the system to reduce volume by shifting toward fewer gas moles. Fritz Haber applied these thermodynamic principles to ammonia synthesis.