Question

Consider the following reversible reaction at equilibrium: c6h12o6 (aq) 6 o2(g) 6 co2(g) 6 h2o(l). given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

Answer 1

Adding heat to an exothermic reaction causes the equilibrium to shift towards the reactants due to Le Chatelier's principle, thereby relieving the stress of the added heat.

Step-by-step explanation:

When heat is added to the equilibrium system C6H12O6 (aq) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(l), which is exothermic, the system will respond according to Le Chatelier's principle. This principle states that if a change is applied to a reaction mixture at equilibrium, the system will adjust to counteract the change and restore equilibrium. Since the reaction is exothermic, adding heat is akin to adding a product of the reaction (in this case, the heat itself). Thus, the system will shift in the direction that absorbs this added heat and reduces its effects. In other words, the equilibrium will shift toward the reactants, which is to the left. The stress caused by the addition of heat is relieved by the reaction moving in the endothermic direction, reducing the concentration of products and increasing the concentration of reactants.