What is the partial pressure of dry air when the partial pressure of water vapor is one atmosphere

First of all, water can exist in three phases in nature: "gas, liquid, and solid". Water also has direct evaporation in the solid state and becomes water vapor.

When water coexists in both gas-liquid phases, vaporization and liquefaction exist at the same time. Under standard atmospheric pressure, the water vapor on the water surface has different saturation partial pressure under different temperature conditions, and when the temperature rises, the saturated partial pressure of water vapor on the water surface is rising, that is, the rate of vaporization is greater than the speed of liquefaction, which can also explain why heating can accelerate the evaporation of water, and liquid water will be lost. Water boils when the saturated partial pressure of water vapor on the surface of the water is equal to the local atmospheric pressure as the temperature increases.

This can also explain why pressure cookers are needed on the plateau, because, at the local atmospheric pressure, at a relatively low temperature, the water will boil, and the temperature of the water will not rise, so it is necessary to cook food in a confined space (the pressure cooker is sealed) by increasing the pressure in the pot to make the water temperature rise. At atmospheric pressure, if the container of water is open, from the moment when water and steam coexist, the process of evaporation and condensation of water and water vapor in order to maintain the dynamic equilibrium of vaporization and liquefaction has always existed, but due to the open container, a part of the water vapor will diffuse into the air, so the water will slowly evaporate and dry, that is, all of it will evaporate.

Partial pressure of air (components other than water) = total pressure - partial pressure of water vapor.

The partial pressure of water vapor refers to the pressure formed by water vapor in moist air. According to Dalton's law, the sum of the partial pressure of water vapor and the partial pressure of dry air is equal to atmospheric pressure.

In moist air, water vapor alone occupies the volume of moist air, and has the same temperature as moist air, the pressure generated, called the partial pressure of water vapor, generally at room temperature in the atmospheric pressure of the water vapor partial pressure accounted for a very low proportion, cold areas are lower than hot and humid areas, winter is lower than summer, but the difference between day and night is not much.

The partial pressure of water vapor decreases with increasing altitude, and its proportion of decline is greater than that of air pressure. The partial pressure of water vapor when the water vapor content of air at a certain temperature reaches saturation is called the saturated water vapor partial pressure at that temperature.

At a certain temperature, the ratio of the partial pressure of water vapor of moist air to the partial pressure of saturated water vapor at the same temperature is relative humidity. Indicates the degree to which water vapor in moist air is close to saturation. The greater the partial pressure of water vapor in the air, the higher the moisture content.

Partial pressure and partial pressure are the same concept, just like the atmospheric pressure, not the atmospheric pressure is the same.

Partial pressure of water vapor p[pa]: The partial pressure of water vapor in moist air at a certain temperature.

Partial pressure of saturated water vapor PSC[PA]: The partial pressure of water vapor when the water vapor in the air is saturated.

Condensation occurs when the partial pressure of water vapor in the air exceeds the partial pressure of saturated water vapor at that temperature and pressure.

The formula for calculating the partial pressure of water vapor in ambient air is:

p h2o = * h 100) *exp [ t ( t + where the unit of temperature is degrees Celsius, the unit of partial pressure is kpa, and the unit difference of relative humidity h is %. exp denotes an e-based index.

Be careful not to make a mistake in the formula. To provide you with a trial correction point: when the relative humidity is 0 degrees Celsius and the relative humidity is 100% (i.e., the saturated state of water vapor in the virtual skin), the partial pressure of the vapor in the water swimming mold should be kpa

When the pressure of the moist air is slowed down, the partial pressure of the water vapor slippery in the water vapor depends on ().

a.Relative humidity.

b.Moisture content.

c.Wet-bulb temperature.

d.Dry-bulb temperature.

Correct Answer: Moisture content.

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The temperature is 3 degrees, the atmospheric pressure is 1000 Pa, and the partial pressure of saturated water vapor is about 1 kiloPa. It can be calculated using the saturated water vapor pressure formula: at 3 degrees, the saturated water vapor pressure is:

e = exp( 3 3 + where e is the partial pressure of saturated water vapor in kPa. Bringing in the calculations, the partial pressure of saturated water vapor is about kPa.

What is the partial pressure of saturated water vapor at a temperature of 3 degrees and an atmospheric pressure of 1000 Pa?

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The temperature is 3 degrees, the atmospheric pressure is 1000 Pa, and the partial pressure of saturated water vapor is about 1 kiloPa. It can be calculated using the saturated water vapor pressure formula: at 3 degrees, the saturated water vapor pressure of the jujube is:

e = exp( 3 3 + where e is the partial pressure of saturated water vapor in kPa. It can be calculated that the partial pressure of saturated water vapor is about kPa.

Hello, There is another question: the law of water vapor with temperature and atmospheric pressure.

What is the partial pressure of saturated water vapor at a temperature of 3 degrees and an atmospheric pressure of 65,200 Pa?

The saturation of the vapor in the water section increases with the increase of temperature, that is, at the same volume, the higher the temperature, the higher the partial pressure of the water vapor. At a certain temperature, if the surface of the water is constant, the water that can be evaporated is also certain, and when the partial pressure of the saturated water vapor pants in the air is equal to the saturated water vapor pressure of the water at that temperature, it is called the saturated state. As the pressure increases, so does the saturated water vapor pressure of the water.

Does atmospheric pressure not affect the partial pressure of saturated water vapor.

Also what is the partial pressure of saturated water vapor at a temperature of 12 degrees and an atmospheric pressure of 103,000 Pa?

You can refer to the saturated water vapor pressure gauge of Minghu Zhengshui, when the temperature is 3 degrees Celsius and the atmospheric pressure is 65200 Pa, the saturated water vapor pressure of the water is Pa. Therefore, under such conditions, the partial pressure of saturated water vapor is Pa.

Is there a table. What kind of watch do you need to kiss?

Does atmospheric pressure not affect the partial pressure of saturated water vapor.

The change in pro-atmospheric pressure affects the partial pressure of saturated water vapor. The partial pressure of saturated water vapor increases with the increase of temperature, which means that if the atmospheric pressure rises at the same temperature of Shinga, the partial pressure of the saturated water vapor slip mode will also increase; Vice versa. This is because, atmospheric pressure affects the kinetic equilibrium of water vapor formation and hence can affect the partial pressure of water vapor.

According to 1MPa = 1000kPa = kg square centimeter), the relationship between saturated vapor pressure (kgf cm2) and steam temperature can be calculated according to the standard table of saturated steam pressure (MPa representation) and steam temperature, as follows:

There is a one-to-one correspondence between the temperature and pressure of saturated steam, and there is only one independent variable between the two. The ideal saturated steam state refers to the one-to-one correspondence between temperature, pressure and vapor density. The steam that has this relationship is saturated steam, and there is a table of saturated steam pressure and temperature.

The standard saturated steam pressure and steam temperature comparison table is compiled according to the International System of Units, i.e. the pressure unit is MPa and the temperature unit is .

If the water is heated at four atmospheres, and the water is heated into a saturated steam state, the steam pressure is also four atmospheres, and the Wu Shen will change the Wu Qi, according to the single value correspondence between the pressure and the saturation temperature, it can be seen that the corresponding saturation temperature is degrees, and the same cavity orange loss is stable, and then continue to heat will become superheated steam, and the temperature will rise.

Atmospheric pressure refers to the pressure value in the air, water vapor pressure refers to the pressure value of water vapor, the lower the atmospheric pressure, the temperature drops, the water will solidify, and the less the vapor pressure.

Water vapor pressure Saturated vapor pressure = relative humidity, the lower the relative humidity, the easier it is for water to evaporate.

The atmosphere is a mixture of gases, mostly nitrogen, and a larger part of oxygen, but also contains small amounts of gases such as carbon dioxide and water vapor.

If the ideal gas model is used, each gas in the gas mixture shares a volume, and each gas has a partial pressure on the container wall, and the more the amount of the gas, the greater its partial pressure, and the total pressure of all gas components is atmospheric pressure.

In thermodynamics, this treatment method is called the Dalton partial pressure principle, which should also be mentioned in chemistry. Water vapor pressure is the partial pressure of the water vapor part of the atmosphere. Obviously, this partial pressure is closely related to the condensation of water vapor.

The macroscopic evaporation of water is actually the common result of two microscopic processes: evaporation and condensation, evaporation is that liquid water molecules run out of the liquid to become water vapor molecules, and condensation is that gaseous water molecules enter the liquid to become liquid water molecules, and the evaporation rate exceeds the condensation rate, which can be called evaporation on a macroscopic scale.

The evaporation rate is equal to the condensation rate, and the water cannot evaporate macroscopically. The evaporation rate is independent of the vapor pressure, but the condensation rate is positively related to the vapor pressure, and when the vapor pressure is saturated vapor pressure, the evaporation rate is equal to the condensation rate.

1. Because the boiling point is defined in this way, there is no why, the definition of boiling point is the temperature when the saturated vapor pressure of the liquid is equal to the external pressure. 2. The vapor pressure is greater than the external atmospheric pressure, and the phenomenon is called boiling, of course, this also belongs to the category of boiling.

You know that air is made up of a lot of gases, and there are many different kinds of gases in the air.

Let's start with an example, in a vacuum-tight container, the pressure is zero, right?

Then, after a certain amount of oxygen V1 is charged, the pressure is assumed to be A;

Then, a certain amount of carbon dioxide V2 is added, and the pressure is b (note that b is the total pressure here); The pressure produced by carbon dioxide is a-b;

a/b=v1/(v1+v2)

This means that it is proportional to the volume.

The pressure of the water vapor contained in the air is the pressure produced by the part of the water vapor contained in the air.