How does the vapor pressure of water at 10 degrees celsius with its vapor pressure at 50 degrees celsius?

Answer 1

Do you mean, how does the pressure of water vapor at 10˚C compare with its pressure at 50˚C?

The vapor pressure of water is the pressure at which steam is saturated. Above this pressure, the water would begin to condense. In a gas mixture saturated with water vapor, the vapor pressure is equal to the partial pressure. The vapor pressure is a function of temperature. Many equations of state can predict vapor pressures of liquids but the best ones are also rather complex and require considerable expertise to use. For most purposes, there are several simpler empirical equations which can estimate the vapor pressures of liquids with sufficient accuracy for most purposes.

One of the simplest is the Antoine equation which has the form:

log10Pvap = A - B/(C+T) where the Pressure (P) is in mmHg and the Temperature (T) is in °C.

For water in the range from 1 °C to 100 °C, the constants have the values:

A = 8.07131

B = 1730.63

C = 233.426

Using these values, the vapor pressure of water can be estimated as:

Pvap(@10 °C) = 9.158817 mmHg

Pvap(@50 °C) = 92.29989 mmHg

... so the vapor pressure of water at 50 °C is roughly 10 times the vapor pressure at 10 °C.

Answer 2

The vapor pressure of water at 10 degrees Celsius is lower than its vapor pressure at 50 degrees Celsius. This is because as the temperature increases, the molecules of water gain more energy and move faster, leading to an increase in vapor pressure.