The latent heat of vaporization of liquid nitrogen is about \(200 . \mathrm{kJ} / \mathrm{kg} .\) Suppose you have \(1.00 \mathrm{~kg}\) of liquid nitrogen boiling at \(77.0 \mathrm{~K}\). If you supply heat at a constant rate of \(10.0 \mathrm{~W}\) via an electric heater immersed in the liquid nitrogen, how long will it take to vaporize all of it? What is the time for \(1.00 \mathrm{~kg}\) of liquid helium, whose heat of vaporization is \(20.9 \mathrm{~kJ} / \mathrm{kg}\) ?

In the realm of physics, thermodynamics is the branch that deals with the relationships between heat and other forms of energy. Specifically in the context of latent heat of vaporization, thermodynamics involves the analysis of energy transfer when a substance changes phases from liquid to gas. Latent heat itself is a form of energy released or absorbed by a substance during a phase change without changing its temperature.

The problem involving liquid nitrogen and helium illustrates an important thermodynamic phenomenon where the substances require a certain amount of heat energy, known as the latent heat of vaporization, to transform from a liquid into a vapor. This energy breaks the intermolecular bonds holding the liquid together, allowing molecules to escape into the air as gas. Each substance has a unique latent heat of vaporization value which is crucial in calculating the time taken for the phase change at a given power input from an electric heater.

Heat transfer is a fundamental concept within thermodynamics and engineering that describes the movement of heat energy from one place to another. It plays a crucial role in the process of vaporization, as heat needs to be continuously supplied for a phase change to happen.

From a practical perspective, when heat is supplied at a constant rate via an electric heater, as in the given exercise, it's essential to understand how this energy input affects the speed of vaporization for different substances. The concept of heat transfer efficiency and the ability of a substance to absorb heat (specific heat capacity) are underlying factors determining the rate at which a liquid will be converted into a gas. In solving the exercise, the step-by-step approach breaks down the transfer process into manageable calculations, allowing students to grasp how time, power and energy interact during vaporization.

A phase change is a transition of matter from one state to another due to a change in the environmental conditions, primarily temperature and pressure. The provided exercise demonstrates a specific phase change—the vaporization of a liquid into gas. Vaporization requires the liquid to gain enough thermal energy to overcome atmospheric pressure and transform into vapor, a process characterized by the latent heat of vaporization.

While working through similar exercises, students can benefit from a deeper understanding of the phase diagram and the Clausius-Clapeyron relation. These concepts provide insight into how different thermodynamic variables are interconnected and affect the phase transitions of substances like nitrogen and helium. Grasping these fundamentals supports more accurate and intuitive predictions about the behavior of materials under varying thermal conditions.