An equilibrium constant ...

A. is small when the products are favored in the reaction.
B. is calculated by dividing the concentration of the reactants by the concentration of the products.
C. is the same, regardless of the initial concentrations of reactants.
D. is independent of temperature.
E. All of these.

Look at the definition of Keq.

In the reaction
A + B ==>C + D
Keq = (C)(D)/(A)(B)
For answer a and b, look at Keq. If C and D are large will Keq be large or small? If A and B are large, will Keq be large or small.
For answer c, how does that fit the definition?
T affects the value of Keq. and answer e is not correct.

DrBob222 you didn't answer the question at all...

the answer's C

The correct answer is E. All of these.

An equilibrium constant (K) is a mathematical expression that describes the relationship between the concentrations (or partial pressures) of the reactants and products at equilibrium for a chemical reaction.

A. When the products of the reaction are favored at equilibrium, the equilibrium constant is small. This is because a small K value indicates that the concentration of products is relatively low compared to the reactants.

B. The equilibrium constant is calculated by dividing the concentration (or partial pressure) of the reactants by the concentration (or partial pressure) of the products. This ratio is determined using the balanced chemical equation for the reaction.

C. The equilibrium constant is independent of the initial concentrations of the reactants. It is solely determined by the stoichiometry of the balanced chemical equation. However, it does depend on temperature.

D. The equilibrium constant is not independent of temperature. It changes with temperature according to the principle called Le Chatelier's principle. Increasing the temperature of an exothermic reaction decreases the equilibrium constant, while increasing the temperature of an endothermic reaction increases the equilibrium constant.

To find the equilibrium constant for a reaction, you need to know the balanced chemical equation and the concentrations (or partial pressures) of the reactants and products at equilibrium. By plugging these values into the equilibrium expression, you can calculate the value of K.