The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) This reaction is Reactant favored at equilibrium. Enter PRODUCT or REACTANT. The concentrations of NH3 and H2S will be at equilibrium. Enter HIGH or LOW.

Answer : The reaction is reactant favored and concentrations of NH₃ and H₂S will be low at equilibrium.

Explanation :

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.

As we know that the concentrations of pure solids and liquids are constant that is they do not change. Thus, they are not included in the equilibrium expression.

The given equilibrium reaction is:

The expression of equilibrium constant is:

There are 3 conditions:

When ; the reaction is product favored.

When ; the reaction is reactant favored.

When ; the reaction is in equilibrium.

As we are given that:

That means,

When then the reaction is reactant favored.

Therefore, the reaction is reactant favored and concentrations of NH₃ and H₂S will be low at equilibrium.

im pretty sure its b

bcde is the incorrect answer it is a