H2O(g) + CO(g) = H2(g) + CO2(g)
Which of the following statements are true and which are false.
a) 1 mol of H2O(g) and 1 mol of CO(g) are placed in a vessel and 1 mol of H2(g) and 1 mol of CO2(g) are placed in another of equal volume. At equilibrium, at 350°C, the amounts of H2O(g) in the two vessels are not equivalent.
b) At equilibrium, the overall composition of the reaction mixture is not changing.
c) Q = K when the system is at equilibrium.
d) At equilibrium, individual molecules may be subject to rapid chemical transformations.
e) Amounts of all reactants and products corresponding to an exact equilibrium composition for this reaction are sealed in a vessel. The CO placed in the vessel is labelled with 14C. After an indefinite period of time 14C may be found in both CO and CO2 molecules.
f) The equilibrium constant does not reveal the rate of that reaction.
f is true.
e is true.
I am unsure how to interpret part d but by my interpretation it is true. Equilibrium is not a static set because even at equilibrium the equation is a dynamic one and the concentrations are changing rapidly. Also see part b and understand that although the system is still dynamic at equilibrium the K for the reaction does not change rapidly and the overall concentrations do not change.
c is true.
a is false. They will be the same.
a) False. At equilibrium, the amounts of H2O(g) in the two vessels would be equivalent if the reaction has reached equilibrium.
b) True. At equilibrium, the overall composition of the reaction mixture remains constant as the forward and reverse reactions occur at equal rates.
c) True. Q = K when the system is at equilibrium. Q represents the reaction quotient while K represents the equilibrium constant.
d) True. At equilibrium, individual molecules may continue to undergo rapid chemical transformations as the forward and reverse reactions occur simultaneously.
e) True. After an indefinite period of time, 14C may be found in both CO and CO2 molecules due to the nature of the reaction and the movement of atoms.
f) True. The equilibrium constant (K) provides information about the position of equilibrium, but it does not reveal the rate at which the reaction occurs. The rate of the reaction is determined by factors such as temperature, concentration, and catalysts.
a) False. According to the balanced equation, 1 mol of H2O(g) and 1 mol of CO(g) react to form 1 mol of H2(g) and 1 mol of CO2(g). At equilibrium, the amounts of H2O(g) in the two vessels would be equivalent since the stoichiometry of the reaction is 1:1.
b) True. At equilibrium, the reaction reaches a dynamic state where the rate of the forward and reverse reactions is equal. As a result, the overall composition of the reaction mixture remains constant.
c) True. The equilibrium constant (K) is the ratio of the concentrations (or partial pressures) of the products to the concentrations (or partial pressures) of the reactants at equilibrium. When the system is at equilibrium, the reaction quotient (Q) is equal to the equilibrium constant (Q = K).
d) True. At equilibrium, individual molecules may continue to undergo rapid chemical transformations, but the overall composition of the reaction mixture remains constant.
e) True. In a closed system, the carbon-14 isotope (14C) present in the initial CO reactant can undergo radioactive decay, producing 14C atoms that can become incorporated into both CO and CO2 molecules. After an indefinite period of time, some of the CO and CO2 molecules will contain 14C.
f) True. The equilibrium constant (K) provides information about the relative concentrations (or partial pressures) of reactants and products at equilibrium but does not provide any information about the rate at which the reaction proceeds in either the forward or reverse direction.
a) False: According to the balanced chemical equation, the stoichiometric ratio between H2O(g) and CO(g) is 1:1. Therefore, when 1 mol of H2O(g) and 1 mol of CO(g) are reacted, they will completely convert into 1 mol of H2(g) and 1 mol of CO2(g). At equilibrium, the amounts of H2O(g) in the two vessels would be equivalent because the reaction has gone to completion.
b) True: At equilibrium, the forward and reverse reactions occur at the same rate, resulting in a balanced composition of reactants and products. The overall composition of the reaction mixture remains constant because there is no net change in the amounts of reactants and products.
c) True: The reaction quotient (Q) is the expression of the reaction's concentrations at any given point in time. When the system is at equilibrium, Q becomes equal to the equilibrium constant (K). Therefore, Q = K when the system is in an equilibrium state.
d) True: At equilibrium, the individual molecules of reactants and products are continuously undergoing chemical transformations. While there is no net change in the overall composition, individual molecules are still participating in both forward and reverse reactions. This dynamic nature of equilibrium allows for rapid chemical transformations at an atomic or molecular level.
e) True: In an equilibrium system, if reactants and products corresponding to an exact equilibrium composition are sealed in a vessel, the reaction will continue to occur but at a balanced rate. This means that the forward and reverse reactions are still happening, resulting in interconversion between CO and CO2. If the CO is labeled with 14C, after a long enough period of time, 14C may be found in both CO and CO2 as they continue to exchange carbon atoms.
f) True: The equilibrium constant (K) gives information about the ratio of products to reactants at equilibrium but tells us nothing about the speed or rate at which the reaction reaches equilibrium. A reaction with a high or low equilibrium constant does not provide any information about the kinetics or the time required for the reaction to reach equilibrium. The equilibrium constant only reflects the extent of the reaction at equilibrium, not the speed at which it gets there.