The value of the equilibrium constant, Kc, at a certain temperature is 2.56 x 10-1. If the reaction quotient for a mixture of these species at the same temperature is found to be 9.90 x 10-4, would the mixture yield more products, more reactants or is it at or near equilibrium? Assume a reaction quotient within a factor of 10 of the equilibrium constant is at equilibrium. Enter P, R or EQ.
CH4(g)+H2O(g) = CO(g)+3H2(g)
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To determine whether the mixture will yield more products, more reactants, or is at or near equilibrium, we need to compare the reaction quotient (Qc) with the equilibrium constant (Kc).
In this case, we are given that the equilibrium constant (Kc) at the given temperature is 2.56 x 10-1.
The reaction quotient (Qc) for the mixture is found to be 9.90 x 10-4.
Comparing Qc with Kc:
- If Qc < Kc, it means the mixture has more reactants than products, and the reaction will proceed in the forward direction to form more products.
- If Qc > Kc, it means the mixture has more products than reactants, and the reaction will proceed in the reverse direction to form more reactants.
- If Qc = Kc, it means the mixture is at equilibrium.
Now, let's compare Qc with Kc:
Qc = 9.90 x 10-4
Kc = 2.56 x 10-1
Since Qc is significantly smaller (by a factor of 10^2) than Kc, we can conclude that the mixture has more reactants than products. Therefore, the reaction will proceed in the forward direction to form more products.
In conclusion, the mixture will yield more products.