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The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant. Q = products/reactants If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium. If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.
Solids and liquids
Molarity of products divided by reactants Keq=(products)/(reactants)
Molarity of products divided by reactants Keq=(products)/(reactants)
Kc is the equilibrium constant.
H2SO3 will ionize to H+ + HSO3-. The Keq = [H+][HSO3-]/[H2SO3]HSO3- will ionize to H+ + SO3^2-. The Keq = [H+][SO^2-]/[HSO3-] ... very small value
Keq= ([A]a[B]b/[C]c[D]d)
K(eq)= 1.33
The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant. Q = products/reactants If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium. If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.
Solids and liquids
Molarity of products divided by reactants Keq=(products)/(reactants)
keq = 1.125
keq = 1.125
Because it means that the equilibrium mixture contains more product than reactants.
Products and reactions are equally favored in the reactions
Molarity of products divided by reactants Keq=(products)/(reactants)
If a reaction creates far more products than reactants, the numerator is large and the denominator is small. That means Keq will be large. So when Keq is large, equilibrium is to the far right of the reaction. A reaction that goes to completion would have an infinite Keq, since the concentration of reactants goes all the way to zero.If few products form, and many reactants remain, the numerator is small and the denominator is large. So a small Keq means that equilibrium is far to the left.you're welcome.