Can Total Energy Be the Same in Liquid and Vapour Phases at Equilibrium?

In summary, the question is asking which option (a. inter-molecule forces, b. potential energy, c. kinetic energy, d. total energy) can be similar between the liquid and vapour phases of a substance in equilibrium. The answer is that the total energy can be the same, as the molecules in both phases have equal total energy. However, the kinetic energy may not necessarily be the same, as energy is required to evaporate a liquid into a vapour.
  • #1
Strawberry1711
4
0

Homework Statement


A liquid is in equilibrium with its vapour at it’s boiling point. On the average, the molecules in the two phases have equal;; provided options are:
a. inter-molecule forces
b.potential energy
c .Kinetic energy
d.total energy

.

Homework Equations

The Attempt at a Solution

:
Answer is Total energy
I am unable to understand that since vapour and liquid phases are in equilibrium that means they are exerting similar pressure which means kinetic energy should be same also how can both of them have same energy if they are in different phases?
Can you please tell me how can total energy be same in this question
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  • #2
It can't. You have to put energy into a liquid to evaporate it.
What is the same between two phases in equilibrium? How is this related to any of the options you are given?
 
  • #3
The question asks for what kind of force / energy can be possibly similar in liquid and vapour phase of the atom/molecule in state of equilibrium.
 

FAQ: Can Total Energy Be the Same in Liquid and Vapour Phases at Equilibrium?

What is liquid and vapor equilibrium?

Liquid and vapor equilibrium is a state in which a liquid and its associated vapor are in a stable balance, meaning that the rate of evaporation is equal to the rate of condensation. This occurs when the pressure and temperature of the system are constant.

How is liquid and vapor equilibrium affected by temperature?

An increase in temperature typically leads to an increase in the equilibrium vapor pressure, as more molecules have enough energy to escape the liquid phase and enter the vapor phase. This results in a higher concentration of vapor in the system and a shift towards the vapor phase.

What is the importance of liquid and vapor equilibrium?

Liquid and vapor equilibrium is important in many industrial and natural processes, such as distillation, evaporation, and boiling. It also plays a crucial role in the formation of clouds and other atmospheric phenomena.

How does pressure affect liquid and vapor equilibrium?

The equilibrium vapor pressure of a liquid increases with an increase in external pressure. This is because the molecules in the vapor phase are compressed, making it more difficult for them to escape back into the liquid phase. As a result, the vapor phase becomes more concentrated and the equilibrium shifts towards the liquid phase.

Can liquid and vapor equilibrium be achieved in an open system?

No, liquid and vapor equilibrium can only be achieved in a closed system where the pressure and temperature remain constant. In an open system, the vapor can escape into the surrounding environment, leading to an imbalance in the equilibrium between the liquid and vapor phases.

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