Final answer:
The forward equilibrium reaction of 2SO2(g) + O2(g) → 2SO3(g) is exothermic and proceeds to form SO3, crucial in sulfuric acid manufacturing. Higher temperatures increase the reaction rate but lower the equilibrium concentration of SO3. Equilibrium adjusts the concentrations of reactants and products until the rate of the forward reaction equals the reverse reaction rate.
Step-by-step explanation:
The equilibrium reaction 2SO2(g) + O2(g) → 2SO3(g) does proceed in the forward direction under certain conditions. The formation of sulfur trioxide (SO3) from sulfur dioxide (SO2) and oxygen (O2) is a crucial step in the manufacture of sulfuric acid. This reaction releases heat, indicating that it is an exothermic process. At higher temperatures, the reaction rate increases, but the equilibrium concentration of SO3 is lower compared to lower temperatures.
To express the reaction rate, you can write expressions in terms of the rate of change of concentration for each species. For instance, the rate of appearance of SO3 would be expressed as the change in concentration of SO3 over time, and similarly for SO2 and O2.
When discussing equilibrium, the reaction quotient (Q) plays a significant role. If the product concentration (like [SO3]) increases, the reaction quotient will adjust until equilibrium is reached. The forward and reverse reactions proceed at the same rate at equilibrium. The equilibrium constant (K) remains constant at a specific temperature but can change with temperature variations. In this case, as the reaction proceeds, the concentration of SO3 decreases and the concentrations of SO2 and O2 increase until the reaction reaches equilibrium.