### 5.6 Koehler Theory

So, now we can put the pieces together. The equilibrium vapor pressure for a water drop containing a solute is simply the triple product of the saturation vapor pressure for pure water over a plane surface, the curvature effect, and the solute effect:

$$\begin{array}{l}{e}_{eq}({n}_{s},r,T)={e}_{s}(T)\cdot \left(1-{\chi}_{s}\right)\cdot \mathrm{exp}\left(\frac{2\sigma}{{n}_{L}R*Tr}\right)\\ {e}_{eq}({n}_{s},r,T)\approx {e}_{s}(T)\cdot \left(1-\frac{Bi{N}_{s}}{{r}_{d}{}^{3}}\right)\cdot \left(1+\frac{{a}_{K}}{{r}_{d}}\right)={e}_{s}(T)\cdot \left(1+\frac{{a}_{K}}{{r}_{d}}-\frac{Bi{N}_{s}}{{r}_{d}{}^{3}}-\frac{{a}_{K}Bi{N}_{s}}{{r}_{d}{}^{4}}\right)\\ {e}_{eq}({n}_{s},r,T)\approx {e}_{s}(T)\cdot \left(1+\frac{{a}_{K}}{{r}_{d}}-\frac{Bi{N}_{s}}{{r}_{d}{}^{3}}\right)\end{array}$$

This equation is called the **Koehler Equation**.** **It gives us the equilibrium vapor pressure that a drop will have for a given drop radius *r _{d}* and given number of moles of solute

*N*. We can see that there are two competing effects: the curvature or Kelvin effect that depends on the inverse of the drop radius, and the solute or Raoult effect that depends on the inverse of the drop radius cubed.

_{s}Remember we talked about the saturation ratio, *S = e/e _{s}*. We also talked about supersaturation,

*s = S – 1= e/e*. We define a new saturation ratio and supersaturation for a particle,

_{s}– 1*S*and

_{k}*s*, where “k” stands for “Koehler.”

_{k}*s _{k}* is defined as follows:

$$\begin{array}{l}{S}_{k}=\frac{{e}_{eq}({n}_{s},r,T)}{{e}_{s}(T)}\approx \left(1+\frac{{a}_{K}}{{r}_{d}}-\frac{Bi{N}_{s}}{{r}_{d}{}^{3}}\right)\\ {s}_{k}={S}_{k}-1=\frac{{a}_{K}}{{r}_{d}}-\frac{Bi{N}_{s}}{{r}_{d}{}^{3}}\end{array}$$

Equation 5.13 is the form of the Koehler Equation that is most often used. Remember, this equation applies to individual drops. Each drop has its own Koehler curve because each drop has its own amount of solute of a given chemical composition. No two Koehler curves are alike, just as no two snowflakes are alike.

Let's look at a graph of this equation. At 20 ^{o}C, *a _{K}* = 1.1 x 10

^{–9}m,

*B*= 4.3 x 10

^{–6}m

^{3}mole

^{–1}, and

*N*is typically in the range of 10

_{s}^{–18}to 10

^{–15}moles.

**Interpretation of the figure:**

*s*is the supersaturation of the particle, not the atmosphere._{k}- At the smallest
*r*(~10s of nm), the Raoult solute effect (_{d}*–1/r*) is stronger than the Kelvin effect._{d}^{3} - As
*r*gets bigger as water is added to the particle, the Kelvin effect (_{d}*+1/r*) starts to win out over the solute term (_{d}*–1/r*). As a result,_{d}^{3}*s*becomes positive._{k} - As
*r*gets very large, then the surface begins to look “flat” and the solution becomes so dilute that the liquid water approaches “pure” and_{d}*s*approaches 0, which means that_{k}*e*approaches_{eq}*e*._{s} *s*is called critical supersaturation. The particle cannot activate and grow into a cloud drop until the atmospheric supersaturation,_{c}*s*, exceeds*s*._{c}*s*occurs at the critical radius_{c}*r*, for activation. Drops that reach this radius can activate and grow into a cloud drop. Those that don’t won’t._{c}- The greater
*N*, the lower_{s}*s*, and the greater_{c}*r*(see next figure)._{c}

The video below (1:35) explains the Koehler Curve Equation in more depth:

#### Check Your Understanding

Note that the supersaturation is less than 0.2% for the smaller particle and less than 0.1% for the larger particle. As cooling occurs, which one will activate first?

**Click for the answer.**

ANSWER: The larger particle, because it has a lower critical supersaturation.

To see what happens to the drop in the atmosphere, we need to compare the Koehler curve for each drop to the ambient supersaturation of the environment. The Koehler curve is the equilibrium supersaturation, *s _{k}*, for each drop and it varies as a function of the drop size. The ambient supersaturation,

*s*, is the amount of water vapor available in the environment. When

*s*=

_{k}*s*, the drop is in equilibrium with the environment. The drop will always try to achieve this equilibrium condition by growing (condensing ambient water vapor) or shrinking (evaporating water) until it reaches the size at which

*s*=

_{k}*s if it can!*Another way to think about

*s*is that it is telling us something about the evaporation rate for each drop size and temperature. For the drop to be in equilibrium with the environment, the condensation rate of atmospheric water vapor must equal the evaporation rate of the drop.

_{k}*If s*<

_{k}*s, then net condensation will occur and the drop will grow*.

*If s*>

_{k}*s, then net evaporation will occur and the drop will shrink*.

Let's look at two cases. In the first case, the ambient supersaturation is always greater than the entire Koehler curve for a drop.

**Interpretation of the figure:**

- The ambient supersaturation does not depend on the radius of the particle and so is a straight line on the graph.
- The basic concept is the particle supersaturation is constrained to the
*s*curve, the particle grows or shrinks in an effort to have_{k}*s*, that is, to have the particle condensation and evaporation be in equilibrium with the environment’s water vapor._{k}= s - If
*s*>*s*, then the condensation of ambient water vapor is greater than the evaporation from the drop no matter what the drop radius is._{c} - The particle continues to grow, becomes a critical nucleus, and then continues to add water and grow into a cloud drop.
- The drop can start at any size and it will grow into a cloud drop as long as the ambient supersaturation is greater than the Koehler curve.

In the second case, the ambient supersaturation intersects the Koehler curve:

**Interpretation of the figure:**

- If
*s < s*and the drop radius is very small, then the drop grows to a radius on the left side of_{c}*s*and stops when_{c}*s*=_{k}*s*. - The drops are called haze drops. They do not nucleate to become cloud drops but instead stay a smaller size. You have probably often seen haze on a warm, moist summer day.
- If a drop finds itself in an environment where
*s*<*s*, (as could happen if the drop's air is mixed with drier air), then the evaporation from the drop would exceed the condensation from the environment and the drop would shrink until_{k}*s*=*s*._{k} - If a drop happens to find itself in an environment where
*s*=*s*, the drop can shrink back into a haze drop or grow into a cloud drop, depending on the drop radius. If_{k}*r*<*r*, then the drop will shrink until it has a radius for which_{c}*s*=*s*. If_{k}*r*>*r*and_{c}*s*=*s*then the drop is in unstable equilibrium and can either grow into cloud drops by adding a water molecule or can shrink all the way back to a haze drop with a radius that matches the radius for_{k},*s*=*s*._{k} - If
*s*=*s*(which is a special case of_{c}*s*=*s*) then the drop will grow to radius_{k}*r*=*r*and then with the random addition of a little water will grow a little bit more so that_{c}*s*<_{k}*s*. At this point, there will be net condensation and the drop will activate and continue to grow.

You can imagine all kinds of scenarios that can happen when there is a distribution of cloud condensation nuclei of different sizes and different amounts of solute. Drops with more solute have lower values for the critical supersaturation and therefore are likely to nucleate first because, in an updraft, the lower supersaturation is achieved before the greater supersaturation. So you can imagine the larger CCN taking up the water first and taking up so much water that the ambient supersaturation drops below the critical supersaturation for the smaller CCN. As a result, the larger CCN nucleate cloud drops while the smaller CCN turns into haze. The moral of the story? If you're a CCN, bigger is better!

#### Quiz 5-3: How cloud drops form.

- Find
**Practice Quiz 5-3**in Canvas. You may complete this practice quiz as many times as you want. It is not graded, but it allows you to check your level of preparedness before taking the graded quiz. - When you feel you are ready, take
**Quiz 5-3**. You will be allowed to take this quiz only**once**. Good luck!