For the following reaction at equilibrium, indicate if the equilibrium mixture contains mostly products, mostly reactants, or both products and reactants.
2H20(g)-><-2H2(g)+O2(g) kc+4x10-48
Technically, everything reacts a little so we always have some products and some reactants. However, from a practical stand point, look at the K and how you write the expression.
Kc = (H2)^2(O2)/(H2O)^2
Kc = 4E-48. That's a VERRRRRRY small number. That means the numbers on top are small and the numbers on the bottom are large. That's the only way you can get a very small number. What does that tell you about the relations?
It tells us that there isn't much product but a lot of reactant. It is mostly reactants.
To determine whether the equilibrium mixture contains mostly products, mostly reactants, or both products and reactants, we need to compare the value of the equilibrium constant (Kc) for the reaction.
In this case, the given equilibrium constant (Kc) is 4x10^(-48). The magnitude of this equilibrium constant is extremely small, indicating that the reaction heavily favors the reactants. Since the equilibrium constant is much closer to zero, it suggests that there are significantly more reactants present at equilibrium compared to products.
Therefore, for the given reaction, the equilibrium mixture contains mostly reactants.