Air conditioners and dehumidifiers are the same machine -- just different exhaust mechanisms. They both remove water from the air, thus reducing actual and relative humidity.
Heaters raise the air temperature, thus reducing the relative humidity (but not, in general, the actual humidity).
Edit to clarify: "relative humidity" is the amount of water in the air as a percentage of the maximum possible capacity. "humidity," or "absolute humidity," is the molar (or other absolute unit) content of water per unit volume of air. The dew point is the temperature at which a given absolute humidity will start to condense out of the air -- thus an indication of the temperature at which the relative humidity equals or exceeds 100%. The dew point is the same everywhere for a given humidity.
You have a 2 liter rigid container, featuring 1 liter of liquid water and, above it, one liter of a mixture of air and water vapor all at 1 atm. The temperature is 20 C, and the partial pressure of the water vapor in the head space is the equilibrium vapor pressure, so that the system is at equilibrium. This is the initial thermdynamic equilibrium state of the system. Start out by determining the partial pressure of air in the head space, the mass of air in the container, and the mass of water. In the ensuing calculations, it is permissible to assume that the partial pressure of the water vapor in the head space is equal to the equilibrium vapor pressure at the liquid temperature and the air is not soluble in the liquid water.
Vapor pressure of water at 20 C = 17.5 torr = 0.023 atm
Partial pressure of air in container at 20 C = 0.977 atm
From ideal gas law, moles of water vapor in head space = 0.00096
Mass of water in head space = 0.017 grams
Total mass of water in container = 1000.017 grams
Moles of air in head space = 0.04066
Mass of air in head space = 1.18 grams
Now you raise the temperature of the system to 50 C and let it equilibrate. What is the partial pressure of water vapor in the head space, and the mass split between the liquid water and water vapor? And what is the partial pressure of the air in the head space? What is the total pressure.
NOW FOR 50 C
Vapor pressure of water at 50 C = 92.5 torr = 0.121 atm
From ideal gas law, mass density of water vapor in head space = 0.0822 g/l = 0.0000822 g/cc
Let x = mass of water in vapor phase
Mass of water in liquid phase = 1000.017-x
Volume of water in container (cc) = $(1000.017-x)+\frac{x}{0.0000822}=2000$
Solving for x : x = 0.0822 grams
Liquid water remaining = 999.93 grams
Volume of vapor = 1.00007
From ideal gas law, partial pressure of air = 1.077 atm
Total pressure = 1.197 atm.
Now try 100 C, 150 C, 200 C, etc.
Best Answer
The dew point temperature depends on 2 parameters: pressure and humidity.
It does not depend on temperature.
You can find it in a diagram where these two lines intersect:
Because that means that you decrease temperature keeping constant pressure. At some point, lowering temperature like that will end up matching the exact point $(P,T)$ for which your actual humidity is the saturated one. Then water starts condensing.
A good way to see it is using the mass mixing ratio, which can be easily written in terms of mol mixing ratio:
$$w=\frac{m_{vap}}{m_{dryAir}}= \frac{n_{vap}}{n_{dryAir}}\cdot \frac{mm_{vap}}{mm_{dry}}\simeq \frac{n_{vap}}{n_{dryAir}}\cdot 0.622$$
So you can say that $ w= \dfrac{n_v}{n_d} \cdot 0.622 $, but the moles ratio is the same as the pressure ratio:
$$w= \dfrac{P_v}{P_d} \cdot 0.622 = \dfrac{P_v}{P-P_v} \cdot 0.622 $$
There is a particular case, when the pressure is the saturated vapor pressure:
$$w_s= \dfrac{P_s}{P-P_s} \cdot 0.622 $$
Relative humidity is strongly related to this. In fact,
$$ \frac{w}{w_s} = \frac{P_v / P_d }{P_s/P_d} = \frac{P_v}{P_s}=RH$$
So, once you are given your three parameters: $(P,T, RH)$, you can go on. Humidity must be given anyhow: RH, w, or whatever, but you need to know humidity.
You'll obviously have your dew point when $w$=$w_s$.
So you have a first equation: $w_s=constant$. What constant? The one you're given initially, initial conditions.
So you have that
$$const= \dfrac{P_s}{P-P_s} \cdot 0.622 $$
and the saturated vapor pressure depends on $T$. A good model is
$$P_s = A\cdot e^{-B/T}$$
So now you decrease temperature with constant pressure until water condenses. That's an extra equation: $P=const$. What constant? The one you're given initially.
So you finally have the equation that
$$w_0= \dfrac{P_s}{P_0-P_s} \cdot 0.622 $$
$$w_0= \dfrac{A\cdot e^{-B/T_d}}{P_0-A\cdot e^{-B/T_d}} \cdot 0.622 $$
You can get $T_d$ from here.
The constants are $A\simeq 2.53\cdot 10^9 mbar$; $B\simeq 5240 K$.