## Boiling Point of Water At High Pressure

### Task number: 1702

Calculate at what temperature water will boil if the outside pressure is 400 kPa. Under standard conditions the atmospheric pressure is 101 325 Pa and the boiling point of water is 373.15 K (100 °C).

Consider the density of water vapor to be constant and equal to 0.8 kg m^{−3}.

#### Hint

To solve this problem it is necessary to use the Clausius–Clapeyron relation in the following form:

\[\frac{\mathrm{d}p}{\mathrm{d}T} = \frac{l_{w}}{T\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) }.\]#### Analysis

We will use the Clausius–Clapeyron relation and we will solve it as a differential equation, calculating the definite integral from the initial pressure to the final pressure and between the two boiling points. We will get a relation between the boiling point and the pressure from this integral.

#### Notation

*p*_{s}= 400 kPa = 4·10^{5}Paoutside pressure *p*_{0}= 101 325 Pastandard atmospheric pressure *T*_{0}= 373.15 Kboiling point of water under standard atmospheric pressure *ρ*_{v}= 0.8 kg m^{−3}density of water vapor *T*_{w}= ?boiling point of water under outside pressure *Found in Physics Reference Tables:**l*_{w}= 2256 kJ kg^{−1}= = 2.256·10^{6}J kg^{−1}specific heat of vaporization of water *ρ*_{w}= 1000 kg m^{−3}water density #### Solution

The boiling point of water increases with increasing pressure. This fact is used for example when pressure cooking. We will use the Clausius–Clapeyron relation to calculate this phenomenon numerically:

\[\frac{\mathrm{d}p}{\mathrm{d}T} = \frac{l_{w}}{T\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) },\]where

*p*is pressure,*T*is thermodynamic temperature,*l*_{w}is specific heat of vaporization of water,*ρ*_{v}is density of water vapor and*ρ*_{w}is water density. This equation describes the phase transition, i.e. the relation between the phase transition point and pressure.We cannot consider the right-hand side of the equation to be constant because the relation between boiling point and pressure is relatively large, due to the big difference between the two densities of the two phases. We will therefore treat it as a differential equation and we will solve it using the method of separation of variables

\[\frac{\mathrm{d}p}{\mathrm{d}T} = \frac{l_{w}}{T\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) } \Rightarrow \mathrm{d}p = \frac{l_{w}}{\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) }\frac{\mathrm{d}T}{T} \]and then we will integrate from

\[\int_{p_{0}}^{p_{s}}\, \mathrm{d}p =\frac{l_{w}}{\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) }\int_{T_{0}}^{T_{w}}{\frac{1}{T}}\, \mathrm{d}T \] \[p_{s}-p_{0} = \frac{l_{w}}{\left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right) }\left[ \ln T\right] _{T_{0}}^{T_{w}} \] \[\frac{\left( p_{s}-p_{0}\right) \left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right)}{l_{w}} = \ln T_{w} - \ln T_{0} \]*p*_{0}(atmospheric pressure) to*p*_{s}(outside pressure) with respect to pressure, and from*T*_{0}(B.P. of water under standard atmospheric pressure) to*T*_{w}(the B.P. of water we are looking for) with respect to temperature. We can consider the specific heat of vaporization of water and both the densities to be constant, therefore we can factor them out of the integrand.Finally, we evaluate the boiling point

\[ \ln T_{w}=\ln T_{0} + \frac{\left( p_{s}-p_{0}\right) \left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right)}{l_{w}},\] \[T_{w} = T_{0}e^{\frac{\left( p_{s}-p_{0}\right) \left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right)}{l_{w}}}.\]*T*_{w}#### Numerical insertion

\[T_{w} = T_{0}e^{\frac{\left( p_{s}-p_{0}\right) \left( \frac{1}{\rho _{v}}-\frac{1}{\rho _{w}}\right)}{l_{w}}} \] \[T_{w}= 373.15\, \cdot \, e^{\frac{\left( 4\cdot{ 10^{5}}-101325\right) \left( \frac{1}{0.8}-\frac{1}{1000}\right)}{2.256\cdot{ 10^{6}}}}\, \mathrm{K}\] \[T_{w} \dot{=} 440\, \mathrm{K}\]#### Answer

The boiling point of water at the given pressure should be approximately 440 K.

#### Comment

The solution isn’t very precise because the density of water vapor is a function of temperature and pressure, which wasn’t taken into account during the calculation.

The boiling point of water can also be determined by the relation of its equilibrium vapor pressure and temperature. That is because a liquid starts to boil when the vapor pressure at a given temperature is equal to the outside pressure. We can find in the Physics Reference Tables that the equilibrium vapor pressure is 4.155·10

^{5}Pa (pressure closest to the pressure given by the assignment) at the temperature of 418 K, which is then the approximate boiling point of water under that pressure.#### Link to an experiment

The fact that the boiling point of water depends on pressure can also be shown experimentally. Simple experiments that show how B.P. of water decreases with decreasing pressure are described here: Dependence of Boiling Point of Water on Pressure.