Consider the reaction: Which of the following statements are true and which are
ID: 706725 • Letter: C
Question
Consider the reaction:
Which of the following statements are true and which are false.
true or false: At equilibrium the rate of the forward reaction is less than the rate of the reverse reaction.
true or false: At equilibrium, the overall composition of the reaction mixture is not changing.
true or false: The equilibrium position is independent of the initial concentrations.
true or false: 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 would still be found only in the CO molecules and not in CO2.
true or false: 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 CO2(g) in the two vessels are not equivalent.
true or false: At equilibrium, individual molecules cannot undergo any chemical reactions.
Explanation / Answer
The reaction attains an equillibrium state , when the forward and reverse reaction rates become equal. At such time the concentration of species do not chnage.
So here :
False : becauseAt equillibrium the rates of forward reaction become equal to the rates of reverse reaction
True : because The concentration of all the species become constant as the rates become equal.
False : because The equillibrium position is dependent on the initial concentration.
False : because The 14C will be found in both the molecules since the reaction has not stopped
True : because The equillibrium will be attained in both the vessels.