For a certain reaction 2A+B⇌C+3D, Keq=4.2×103, 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.
2 Answers
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Explanation:
The reaction lies to the right side because of the following:
The expression of the equilibrium constant
Since
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:
Keq=[products][reactants]=[C][D]3[A]2[B]=4.2×103
(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