Chemistry
Chemistry
Problem
Carbon monoxide reacts reversibly with nitrogen dioxide to form carbon dioxide and nitrogen monoxide in the gas phase, as represented below. CO(g) + NO₂(g) ⇌ CO₂(g) + NO(g) At a particular instant in an isothermal reaction vessel, the following rate data are obtained: • Rate for the forward process (reactants → products): 1.1 × 10⁻⁴ mol·L⁻¹·s⁻¹ • Rate for the reverse process (products → reactants): 3.3 × 10⁻⁵ mol·L⁻¹·s⁻¹ Respond to the tasks that follow. (a) Calculate the numerical value (with units) of the net rate of conversion for the overall reaction at this instant. Use the sign convention that a positive value corresponds to a net formation of products. (b) Based on your calculation, state whether the system is shifting toward the product side, toward the reactant side, or is at equilibrium at this instant.Intuitive explanation
At any moment in a reversible reaction, the forward and reverse rates tell you whether the system is at equilibrium or shifting toward it. Right now, the forward rate exceeds the reverse rate, so the reaction is proceeding net in the forward direction—the system hasn't reached equilibrium yet. The key insight is that the difference between these rates is the net rate of reaction, which determines how fast concentrations are actually changing and in which direction the equilibrium position will shift.
Intuitive explanation
At any moment in a reversible reaction, the forward and reverse rates tell you whether the system is at equilibrium or shifting toward it. Right now, the forward rate exceeds the reverse rate, so the reaction is proceeding net in the forward direction—the system hasn't reached equilibrium yet. The key insight is that the difference between these rates is the net rate of reaction, which determines how fast concentrations are actually changing and in which direction the equilibrium position will shift.