The Kc for the following reaction at 940oC is 1.38.
Given the concentrations [CO2] = 0.500 M, [H2] = 0.425 M, [CO] = 0.610 M and [H2O] = 0.695 M, one can conclude that:
H2(g) + CO2(g) ↔ CO(g) + H2O(g)
Question 8 options:
A) the system is not at equilibrium and the reaction will proceed to the right
B) the system is at equilibrium and no net change will occur
C) the system is not at equilibrium and the reaction will proceed to the left
D) there is insufficient information to determine which way the reaction will proceed
the answer is c
To determine which way the reaction will proceed, we need to compare the calculated Qc, the reaction quotient, to the given equilibrium constant Kc.
The reaction quotient Qc is calculated by taking the product of the concentrations of the products and dividing by the product of the concentrations of the reactants, each raised to the power of its stoichiometric coefficient. In this case, the reaction is:
H2(g) + CO2(g) ↔ CO(g) + H2O(g)
Qc = [CO] * [H2O] / ([CO2] * [H2])
Substituting the given concentrations:
Qc = (0.610 M) * (0.695 M) / ((0.500 M) * (0.425 M))
= 0.4259
Comparing Qc (0.4259) to Kc (1.38), we can conclude that Qc < Kc. Since Qc is smaller than Kc, it means that the reaction is not at equilibrium.
Therefore, the correct answer is:
C) the system is not at equilibrium and the reaction will proceed to the left
Calculate Q for the reaction using the concns given and compare with Keq.
To determine the direction in which the reaction will proceed, we need to compare the calculated reaction quotient, Qc, with the equilibrium constant, Kc.
The reaction quotient, Qc, is calculated using the same expression as the equilibrium constant, Kc. However, the concentrations used in Qc are not necessarily at equilibrium.
The expression for Qc for the reaction H2(g) + CO2(g) ↔ CO(g) + H2O(g) is:
Qc = [CO][H2O] / ([H2][CO2])
Given the concentrations of [CO2] = 0.500 M, [H2] = 0.425 M, [CO] = 0.610 M, and [H2O] = 0.695 M, we can substitute these values into the expression to calculate Qc:
Qc = (0.610)(0.695) / ((0.425)(0.500))
Qc = 0.425
Now, we compare Qc with Kc. Given that Kc for this reaction is 1.38, we can make the following conclusions:
If Qc < Kc, it means the system is not at equilibrium and the reaction will proceed in the forward direction to reach equilibrium. In this case, Qc = 0.425 < Kc = 1.38, so the system is not at equilibrium and the reaction will proceed to the right.
Therefore, the correct answer is:
A) the system is not at equilibrium and the reaction will proceed to the right.