For a certain reaction #2A + B rightleftharpoons C + 3D#, #K_(eq) = 4.2 xx 10^3#, which of the following is true?
#a)# The reaction is product-favored.
#b)# The reaction rate is fast.
#c)# There are more reactants than products.
#d)# The reaction is neither product-favored nor reactant-favored.
The reaction lies to the right side because of the following:
The expression of the equilibrium constant
Here is a video that I recently made about this topic:
Chemical Equilibrium | Reaction Quotient & Application of a Large K.
The equilibrium constant for this reaction is:
#"K"_(eq) = \frac(["products"])(["reactants"]) = \frac([C][D]^3)([A]^2[B]) = 4.2xx10^3#
(b) We cannot say what the rate of reaction is, because that's a kinetic description of a reaction whose kinetic quantities are unstated. We only know the equilibrium constant, which is a thermodynamic quantity.
(c) This is backwards. If you had more reactants than products, then
(d) This is only true if