Could somebody tell me dose my answer for this question right or wrong for this question.My answer is reverse
2SO2(g) + O2(g) ↔ 2SO3(g)
which has Kp = 3.45 x 106 at 600K.
In an experiment, SO3 at pressure 125 atm is mixed with SO2 at pressure 0.13 atm and O2 at pressure 0.025 atm. Which direction will the reaction proceed to reach equilibrium?
Question 3 options:
1) forward
2) reverse
3) no change
Qp = (SO3)^2/(SO2)^2(O2) = 3.70E7 so reverse is correct.
To determine the direction in which the reaction will proceed to reach equilibrium, you can compare the current reaction quotient (Q) to the equilibrium constant (Kp).
The reaction quotient, Q, is calculated in the same way as the equilibrium constant, Kp, but using the partial pressures of the reactants and products at a given moment instead of the equilibrium concentrations.
In this case, the reaction is: 2SO2(g) + O2(g) ↔ 2SO3(g)
The reaction quotient, Q, is calculated as follows:
Q = (P(SO3))² / (P(SO2))² * (P(O2))
Given the pressures:
P(SO3) = 125 atm
P(SO2) = 0.13 atm
P(O2) = 0.025 atm
Substituting these values into the reaction quotient equation, we have:
Q = (125)² / (0.13)² * (0.025) ≈ 1.356 x 10^7
Comparing Q to the equilibrium constant, Kp, which is 3.45 x 10^6, we see that Q is larger than Kp. This means that there is an excess of products at the current moment.
To achieve equilibrium, the reaction will shift in the reverse direction (option 2). It will favor the formation of reactants and reduce the concentration of products until Q equals Kp.