Choose all of the following statements about the equilibrium constant K that are true:
(a) If the K value for a reaction is > 1 then Go must be negative for this reaction
(b) A large value for K implies there is a strong driver for the reaction to proceed in the forward direction and the reaction will be rapid
(c) If Q is greater than K at a given time of reaction, then the reaction will be moving to the side of more reactants
(d) Q can never exactly equal K
(e) None of these is true
help me!
a) Look at Go = -RTlnK. If K >1 what's the sign of Go?
b)It DOES imply a strong driver for the reaction BUT ".....and the reaction will be rapid" it has nothing to do with the speed. We can have huge K values but the reaction proceeds so slow it will take centuries to complete.
c). If Q>K, that means products are too high and reactants are too low, so ....
d)Of course Q can equal to K.
e. ..
Repost telling me what you are confused about if you still have trouble.
To determine which statements about the equilibrium constant K are true, let's analyze each option:
(a) If the K value for a reaction is > 1, then ΔG° (standard free energy change) must be negative for this reaction.
To assess the truth of this statement, we need to recall the relationship between ΔG° and K. The equilibrium constant (K) is related to the standard free energy change (ΔG°) of a reaction through the following equation:
ΔG° = -RT ln(K)
If K > 1, then the exponent of e in the equation must be negative, suggesting that ΔG° is negative. Therefore, statement (a) is true.
(b) A large value for K implies there is a strong driver for the reaction to proceed in the forward direction and the reaction will be rapid.
To check the validity of this statement, we need to understand the interpretation of the equilibrium constant. A large value of K signifies that the ratio of products to reactants at equilibrium is high, indicating that the reaction strongly favors the formation of products. However, the value of K does not provide information about the rate at which the reaction occurs. Therefore, statement (b) is false.
(c) If Q is greater than K at a given time of reaction, then the reaction will be moving to the side of more reactants.
To evaluate this statement, we need to comprehend the concept of reaction quotient (Q). The reaction quotient is used to determine the direction of the reaction before it reaches equilibrium and is calculated in the same way as the equilibrium constant but using concentrations or pressures at a specific time during the reaction.
When Q > K, it suggests that the ratio of reactants to products is larger than the equilibrium ratio. To restore equilibrium, the reaction will shift in the direction that consumes the excess reactants and forms more products. Therefore, statement (c) is true.
(d) Q can never exactly equal K.
According to the nature of equilibrium, when a system reaches equilibrium, Q is equal to K. At equilibrium, the forward and reverse reactions occur at the same rate, resulting in a constant value for the reaction quotient. Therefore, statement (d) is false.
Summing up the analysis:
(a) True,
(b) False,
(c) True,
(d) False.
Therefore, the correct answer is:
(e) None of these is true.