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What happens if K is very small?

If K is a small number, it means that the equilibrium concentration of the reactants is large. In this case, the reaction as written will proceed to the left (resulting in an increase in the concentration of reactants)

chem.libretexts.org - 15.4: The Magnitude of an Equilibrium Constant - Chemistry LibreTexts

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The equilibrium expression for the synthesis of ammonia

[ce{ 3 H2(g) + N2(g) -> 2 NH3(g)} label{15.4.1}]

can be expressed as

[ K_p =dfrac{P^2_{NH_3}}{P_{N_2}P^3_{H_2}} label{15.4.2}]

or

[ K_c = dfrac{[NH_3]^2}{[N_2] [H_2]^3} label{15.4.3}]

so (K_p) for this process would appear to have units of atm–2, and (K_c) would be expressed in mol–2 L2. And yet these quantities are often represented as being dimensionless. Which is correct? The answer is that both forms are acceptable. There are some situations (which you will encounter later) in which K’s must be considered dimensionless, but in simply quoting the value of an equilibrium constant it is permissible to include the units, and this may even be useful in order to remove any doubt about the units of the individual terms in equilibrium expressions containing both pressure and concentration terms. In carrying out your own calculations, however, there is rarely any real need to show the units. Strictly speaking, equilibrium expressions do not have units because the concentration or pressure terms that go into them are really ratios having the forms (n mol L–1)/(1 mol L–1) or (n atm)/(1 atm) in which the unit quantity in the denominator refers to the standard state of the substance; thus the units always cancel out.

Strictly speaking, equilibrium expressions do not have units.

For substances that are liquids or solids, the standard state is just the concentration of the substance within the liquid or solid, so for something like (ce{CaF(s)}), the term going into the equilibrium expression is ([ce{CaF2}]/[ce{CaF2}]) which cancels to unity; this is the reason we do not need to include terms for solid or liquid phases in equilibrium expressions. The subject of standard states would take us beyond where we need to be at this point in the course, so we will simply say that the concept is made necessary by the fact that energy, which ultimately governs chemical change, is always relative to some arbitrarily defined zero value which, for chemical substances, is the standard state.

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