Question

At equilibrium, a⇌b+3c+d, and the mole ratio of d to b is 1. If the reaction is completed in a 5 L flask, the equilibrium constant (Kc) is:

a) Less than 1
b) Equal to 1
c) Greater than 1
d) Cannot be determined with the given information

Answer 1

Given the stoichiometry of the reaction and the mole ratio, the equilibrium constant (Kc) is likely greater than 1 because the concentration of products is seemingly higher than that of reactants. So the correct answer is option C.

Step-by-step explanation:

The question at hand involves determining the equilibrium constant (Kc) for the reversible reaction a⇌b + 3c + d, given the mole ratio of d to b is 1 at equilibrium. To deduce whether Kc is less than, equal to, or greater than 1, we can analyze the stoichiometry and the relationship between products and reactants.

Since the molar ratios of products to reactants are 1:1 for d to b and 3:1 for c to a, we can infer that for every mole of a that reacts, 4 moles of product (1 b + 3 c + 1 d) are formed. Given this, the concentration of products seems to be greater than that of reactants.

As the Kc expression for this reaction is [b][c]3[d]/[a], and the concentrations of the products are higher, the value of Kc is likely to be greater than 1. Without the exact concentrations, however, we cannot calculate a precise value for Kc, but we can conclude that with high product concentrations relative to reactants, Kc would indeed be greater than 1.