The equilibrium constant is equal to 5.00 at 1300K for the reaction
2SO2(g) + O2(g) <--> 2SO3(g)
if initial concentrations are
[SO2] = 6.00M, [O2] = 0.45M,
[SO3]= 9.00M, the system is
a/. At equilibrium
b/. Not at equilibrium and will remain in an un equilibrated state
c/. Not at equilibrium and will shift to the left to achieve an equilibrium state
d/. Not at equilibrium and will shift to the right to achieve an equilibrim state.
Since you quote concentrations I assume the K of 5.00 is Kc.
Then
Kc = 5.00 = (SO3)^2/(SO2)^2(O2)
Qc = (9.00)^2/(6.00)^2(0.45) = 5.00
Since Qc = Kc, the system is in equilibrium.
Can I just say how much I admire this reaction's determination to achieve equilibrium? It's like the Little Engine That Could. "I think I can, I think I can." But let's see what's really going on here.
To determine if the system is at equilibrium, we need to compare the given concentrations with the equilibrium concentrations. If they're the same, then the system is at equilibrium.
Now, the equilibrium constant (K) is equal to the ratio of products to reactants, raised to the power of their respective stoichiometric coefficients. In this case, K = [SO3]^2 / ([SO2]^2 * [O2]).
So, let's plug in the given concentrations:
K = (9.00M)^2 / ((6.00M)^2 * 0.45M)
K = 9.00M^2 / 5.40M^2
K ≈ 1.50
Since the equilibrium constant is 5.00 and the calculated value is approximately 1.50, we can conclude that the system is not at equilibrium.
To figure out which direction the reaction will shift to achieve equilibrium, we can compare the calculated value of K to the actual value of K. If K is greater than the calculated value, then the reaction will shift to the right. If K is smaller, it will shift to the left.
In this case, the actual value of K is 5.00, which is greater than the calculated value of 1.50. So, the reaction will shift to the right to achieve equilibrium.
Therefore, the correct answer is:
d/. Not at equilibrium and will shift to the right to achieve an equilibrium state.
To determine the state of the system, we need to compare the concentrations of the reactants and products to their respective equilibrium concentrations.
The equilibrium constant (K) is given as 5.00. This means that at equilibrium, the ratio of the product concentrations (SO3^2-) raised to the power of its coefficient (2) is equal to 5 times the ratio of the reactant concentrations (SO2 and O2) raised to their respective coefficients (2 and 1).
The initial concentrations given are [SO2] = 6.00M, [O2] = 0.45M, and [SO3] = 9.00M.
To determine if the system is at equilibrium, we can calculate the reaction quotient (Q) using the initial concentrations:
Q = ([SO3]^2) / ([SO2]^2 * [O2])
= (9.00^2) / (6.00^2 * 0.45)
= 4.50 / 12.15
= 0.37
Since Q ≠ K, the system is not at equilibrium.
To determine the direction in which the system will shift to achieve equilibrium, we compare Q to K:
If Q < K, the reaction has more reactants than products, and the system will shift to the right to reach equilibrium.
If Q > K, the reaction has more products than reactants, and the system will shift to the left to reach equilibrium.
In this case, Q = 0.37, and K = 5.00. Since Q < K, the system is not at equilibrium and will shift to the right to achieve an equilibrium state. Therefore, the correct answer is d/.
To determine the state of the system, we need to compare the calculated Q value with the given equilibrium constant (Kc).
Q is the reaction quotient, which is calculated using the concentrations of the reactants and products at a specific point in time. It has the same form as the equilibrium expression but is not necessarily equal to the equilibrium constant Kc.
To calculate Q, substitute the given initial concentrations into the equilibrium expression:
Q = ([SO3]^2) / ([SO2]^2 * [O2])
Q = (9.00^2) / (6.00^2 * 0.45)
Q ≈ 2.25
Now, let's compare Q and Kc to determine the state of the system:
a/. At equilibrium:
If Q = Kc, then the system is at equilibrium. In this case, Q = 2.25 and Kc = 5.00, so the system is not at equilibrium. Thus, option a is incorrect.
b/. Not at equilibrium and will remain in an un equilibrated state:
If Q ≠ Kc, then the system is not at equilibrium, and it will stay in an un equilibrated state. Since Q ≠ Kc in this case, option b is incorrect.
c/. Not at equilibrium and will shift to the left to achieve an equilibrium state:
If Q < Kc, the system will shift to the right to reach equilibrium. However, since Q > Kc (2.25 > 5.00) in this case, option c is incorrect.
d/. Not at equilibrium and will shift to the right to achieve an equilibrium state:
If Q > Kc, the system will shift to the left to reach equilibrium. Since Q > Kc (2.25 > 5.00), the system is not at equilibrium and will shift to the left to achieve an equilibrium state. Therefore, option d is the correct answer.
In summary, the system is not at equilibrium and will shift to the left to achieve an equilibrium state.