2H2 (g) + O2 (g) ↔ 2H2O (g) + energy (heat)
6. When the reaction between hydrogen and oxygen reaches equilibrium: a. Does the number of molecules in the reaction vessel change? Explain.
b. Is the reaction still proceeding in the forward direction?
c. Is the reaction still proceeding in the reverse direction?
d. Are the concentrations of the products and reactants changing? e. Are the rates of the forward and reverse reactions the same?
f. Does the heat content of the system become constant?
a. No, the number of molecules in the reaction vessel does not change at equilibrium. This is because the forward and reverse reactions are occurring at equal rates, resulting in a constant number of molecules in the system.
b. Yes, the reaction is still proceeding in the forward direction at equilibrium. However, the rate of the forward reaction is equal to the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products.
c. Yes, the reaction is still proceeding in the reverse direction at equilibrium. Similar to the forward reaction, the rate of the reverse reaction is equal to the rate of the forward reaction, resulting in no net change in the concentrations of reactants and products.
d. No, the concentrations of the products and reactants are not changing at equilibrium. The rates of the forward and reverse reactions are equal, leading to a constant concentration of all species involved in the reaction.
e. Yes, the rates of the forward and reverse reactions are the same at equilibrium. This is because the reaction has reached a balance between the forward and reverse reactions, resulting in a steady-state where the rates of the forward and reverse reactions are equal.
f. Yes, the heat content of the system becomes constant at equilibrium. This is because the forward and reverse reactions are occurring at equal rates, and any energy released or absorbed by the reaction is balanced, resulting in a constant heat content in the system.