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 at equilibrium, the rates of the forward and reverse reactions are equal, and therefore the number of reactant molecules converting into product molecules is the same as the number of product molecules converting back into reactant molecules.
b. Yes, the reaction is still proceeding in the forward direction at equilibrium. This means that there are still molecules of hydrogen and oxygen combining to form water.
c. Yes, the reaction is still proceeding in the reverse direction at equilibrium. This means that there are still molecules of water decomposing to form hydrogen and oxygen.
d. The concentrations of the products and reactants are not changing at equilibrium. However, this does not mean that the concentrations are equal. The concentrations of reactants and products reach a constant value at equilibrium.
e. Yes, at equilibrium, the rates of the forward and reverse reactions are equal. This means that the rate of the forward reaction is the same as the rate of the reverse reaction.
f. Yes, at equilibrium, the heat content of the system becomes constant. This is because the forward and reverse reactions are occurring at equal rates, and there is no net energy change in the system.