In this article, we are going to learn what is the difference between the vapor pressure and the boiling point with detailed insights.

**The vapor pressure and boiling point graph shows an exponential curve and denotes the saturation of vapor pressure too. Here is a table below differentiating the vapor pressure vs boiling point:-**

Vapor Pressure | Boiling Point |

The vapor pressure measures the number of vapors present in the system under consideration | The boiling point deals with the temperature of the liquid up to which its temperature can rise |

Vapor pressure measures the pressure due to vapors | The boiling point measures the temperature of the liquids |

The vapor pressure is exerted due to the change of phase from liquid to the vapor | The boiling point is responsible for the phase change |

The vapor pressure leads to the condensation of the vapor to the liquid state | At a boiling point, the liquid evaporates into the gaseous state |

It is a force exerted on the system due to the molecules of vapor | At a boiling point, the vapor pressure is equal to the atmospheric pressure |

It is seen for both solid as well as liquid states | It is related to only the liquid matters |

The vapor pressure can be calculated for a system kept at a constant temperature | The boiling point of a liquid is calculated by keeping the pressure constant |

Vapor pressure varies with the temperature of the system | The boiling point changes with the pressure conditions |

The kinetic energy of the particle is converted to the potential energy gradually | The potential energy is converted into the kinetic energy on an immense supply of heat energy |

The process of rising in vapor pressure is called vaporization | Supplying heat to the liquid rigorously will raise the temperature of the liquid to the boiling point |

**Vapor Pressure And Boiling Point Graph**

**The boiling point is nothing but the temperature at which the phase change occurs and the vapor pressure attains the highest value at that fixed atmospheric pressure.** Hence let us plot a graph of vapor pressure v/s the temperature for a liquid boiling at a constant pressure condition.

The graph of vapor pressure v/s temperature shows the exponential curve as the number of vapors escaping from the liquid overcoming the attractive intermolecular bonds doubles at every rise in temperature of the liquid.

The point TBP denotes the boiling point of the particular liquid on the x-axis, beyond the boiling point of the liquid, the temperature of the liquid does not rise further but only the phase change from liquid to vapors takes place. The point on the y-axis V_{sat} represents the saturation point of the vapor pressure. As the vapors evaporated cool down and condense back into the liquid form. The vapor pressure is maintained constant after reaching the boiling point of the liquid.

**How to Calculate Boiling Point from Heat of Vaporization?**

The heat of vaporization is the amount of heat energy required to transform the liquid state of matter into the gaseous state.

**The boiling point of a liquid can be calculated from heat of vaporization by using the Clausius – Clapeyron equation given as [latex]ln\left ( \frac{P_2}{P_1} \right )=\frac{-\Delta H_{vap}}{R}\left ( \frac{1}{T_2}-\frac{1}{T_1} \right )[/latex].**

**What is the boiling point of water in the pressure cooker which functions at 1.8 bar if the heat of vaporization of water is 45k J/mol?**

**Given: **P_{2}= 1.8 bar

The water at a normal atmospheric condition that is at 1 atm, boils at 100^{0}C, hence

P_{1}= 1 bar

T_{1} =100^{0}C=373.2K

[latex]\Delta H_{vap}=45k\ J/mol[/latex]

Using the Clasius – Clapeyron equation

[latex]ln\left ( \frac{P_2}{P_1} \right )=\frac{-\Delta H_{vap}}{R}\left ( \frac{1}{T_2}-\frac{1}{T_1} \right )[/latex]

[latex]ln\left ( \frac{1.8}{1} \right )=\frac{-45000}{8.314}\left ( \frac{1}{T_2}-\frac{1}{373.2} \right )[/latex]

[latex]ln\left ( 1.8 \right )=-5412.56\left ( \frac{1}{T_2}-0.0027 \right )[/latex]

[latex]0.5878=-5.412\left ( \frac{1}{T_2}-0.0027 \right )[/latex]

[latex]-10.86 \times 10^{5}=\frac{1}{T_2}-0.0027[/latex]

[latex]\frac{1}{T_2}=-10.86 \times 10^{5}-0.0027 [/latex]

[latex]\frac{1}{T_2}=0.00257 [/latex]

[latex]T_2=\frac{1}{0.00257}=389.1 K[/latex]

And 389.1K = 115.9^{0}C

Hence the boiling point of water inside the pressure cooker is 115.90C.

**How to find Boiling Point from Vapor Pressure?**

The boiling point can be found by measuring the saturated vapor pressure developed at that temperature.

**The liquid can have varied boiling points at different pressure in the system. The vapor pressure can be found using the Clausius – Clapeyron equation, also from the phase diagrams, and from the graph of vapor pressure v/s temperature too.**

**What is the boiling point of methane at vapor pressure equal to 2 atm? Given the heat of vaporization of methane is 8.20k J/mol.**

At normal atmospheric pressure, the boiling point of methane is -161.5^{0}C.

P_{1} =1atm

P_{2} =2atm

T_{1} =-161.5^{0}C =-161.5+273.2 =111.7K

[latex]\Delta H_{vap}=8.2k\ J/mol[/latex]

Using Clausius – Clapeyron equation

[latex]ln\left ( \frac{P_2}{P_1} \right )=\frac{-\Delta H_{vap}}{R}\left ( \frac{1}{T_2}-\frac{1}{T_1} \right )[/latex]

[latex]ln\left ( \frac{2}{1} \right )=\frac{-8200}{8.314}\left ( \frac{1}{T_2}-\frac{1}{111.7} \right )[/latex]

[latex]ln\left ( 2 \right )=-986.3\left ( \frac{1}{T_2}-\frac{1}{111.7} \right )[/latex]

[latex]0.6931=-986.3\left ( \frac{1}{T_2}-0.00895 \right )[/latex]

[latex]70.3\times 10^{-5}=-\left ( \frac{1}{T_2}-0.00895 \right )[/latex]

[latex]70.3\times 10^{-5}=0.00895-\frac{1}{T_2}[/latex]

[latex]\frac{1}{T_2}=0.00895-70.3\times 10^{-5}[/latex]

[latex]\frac{1}{T_2}=0.00825[/latex]

[latex]T_2=\frac{1}{0.00825}[/latex]

[latex]T_2=121.2K[/latex]

This is equal to -152^{0} C.

Hence the boiling point of the methane at the vapor pressure of 2 atm increases to -152^{0} C.

**Frequently Asked Questions**

**What are the factors affecting the vapor pressure of the liquid?**

The vapor pressure is due to the pressure felt on the area by the vapors evaporated from the system into the surrounding.

**The most vital factor on which the vapor pressure depends is the temperature and the heat energy supplied to the liquid. Also, the chemical composition and the impurities added will vary the vapor pressure.**

**How vapor pressure depends upon the intermolecular bonding between the atoms?**

On supplying heat energy to the liquid, the intermolecular bonding between the atoms breaks, and particles move in random motion.

**If this intermolecular bonding between the atom in case of a certain liquid is low, which means there is a weak force of attraction between the atoms then these bonds will easily break down will even a small amount of energy supplied to the liquid and thus vapor pressure will be high at small temperature.**

**How are the boiling point and the vapor pressure related to each other?**

The vapors are the result of the rising temperature of the liquid supplying heat.

**At a boiling point, the liquid phase is converted to the gaseous phase and at this temperature, the vapor pressure formed becomes equal to the atmospheric pressure.**