Question

What may be expected when K > 1.0?

Answer 1

The two correct statements are:

1. The concentration of one or more of the products is small

2. The reaction will proceed to the right and favor the formation of products.

LeChatelier's Principle states that when a stress is imposed on a system at equilibrium, the equilibrium will shift to counteract the change. A reduction in the number of products cause the system to respond by making more product, which leads to K>1 and products being more favorable.

Answer 2

Answer: The two correct statements are the concentration of one or more of the reactants is small and the reaction will proceed to the right and favor the formation of products.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power its stoichiometric coefficients. It is expressed as $K_{eq}$

For a general chemical reaction:

$aA+bB\rightarrow cC+dD$

The expression for $K_{eq}$ is given as:

$K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

Equilibrium constant is inversely related to the concentration of the reactants. So, if concentration of any reactants is less, the vale of $K_{eq}$ will be more.

Conditions of $K_{eq}$ are:

• When K < 1; the reaction is favored to the left or in backward direction or reactants are formed more.
• When K > 1; the reaction is favored to the right or in forward direction or products are formed more.
• When K = 1; the reaction is in equilibrium.

Hence, the two correct statements are the concentration of one or more of the reactants is small and the reaction will proceed to the right and favor the formation of products.