Final answer:
Increasing the temperature during the Haber process shifts the equilibrium towards the reactants, decreasing the production of ammonia (NH3) and increasing the concentrations of nitrogen (N2) and hydrogen (H2).
Step-by-step explanation:
When the temperature is increased during the Haber process, the equilibrium shifts in favor of the reactants. The Haber process is an exothermic reaction, meaning it releases heat. According to Le Chatelier's principle, increasing the temperature adds heat to the system, which favors the endothermic reverse reaction where heat is absorbed. Therefore, the concentration of ammonia (NH3) decreases while the concentrations of nitrogen (N2) and hydrogen (H2) increase.
An increase in temperature causes a shift in equilibrium that reduces the value of the equilibrium constant (Keq) for exothermic reactions. As a result, a higher temperature decreases ammonia production in the Haber process. Conversely, lowering the temperature favors the forward reaction and increases ammonia concentration, as the system shifts to release heat.