Back to Portal
Class 9Science
RHS Logo
Published 2026-08-29•Chapter: Matter in Our Surroundings

Matter in Our Surroundings - States of matter, factors affecting evaporation, and latent heat

Master Guide: States of Matter, Latent Heat, and Evaporation

Hello students! Welcome to today’s lesson. Have you ever wondered why ice melts into water, why steam burns more than boiling water, or why water stored in a traditional earthen pot (*matka*) stays so refreshingly cool during hot Indian summers?

All these everyday phenomena are governed by the fascinating principles of chemistry found in Chapter 1 of your NCERT Science textbook: Matter in Our Surroundings.

In this tutorial, we will break down three crucial core topics:

  • The Three States of Matter
  • The Mystery of Latent Heat
  • Evaporation and Factors Affecting It

    • Grab your notebooks, and let’s make these concepts crystal clear!

    ---

    Part 1: The Three States of Matter

    Everything around us—from the air we breathe to the water we drink and the bench you are sitting on—is made up of matter. Matter is anything that has mass and occupies space (volume).

    Matter is made up of tiny particles. The arrangement and behavior of these particles determine whether matter exists as a solid, a liquid, or a gas.

    The Particle Picture: Real-World Analogy

    Imagine a school assembly:

  • Solids: Students standing in strict, tight rows, holding hands firmly. They can only wiggle in place; they cannot move away.
  • Liquids: Students holding hands loosely, sliding past one another inside a marked area. They have some freedom to move.
  • Gases: Students running freely all over a huge playground, completely independent of one another, constantly colliding!

    • ---

    Comparison of the Three States

    PropertySolidLiquidGas
    ShapeFixed shapeTakes the shape of the containerNo fixed shape
    VolumeFixed volumeFixed volumeNo fixed volume (expands to fill container)
    Inter-particle SpaceExtremely small (particles tightly packed)Moderate (particles loosely packed)Very large (particles far apart)
    Force of AttractionMaximumMediumMinimum (negligible)
    Kinetic Energy of ParticlesLowest (particles only vibrate)ModerateHighest (particles move randomly at high speed)
    CompressibilityNegligibleVery lowHigh (e.g., LPG cylinders, CNG)
    Teacher's Tip for Exams: NCERT often asks why gases exert pressure on the walls of a container.
    Answer: In the gaseous state, particles move about randomly at high speeds. Due to this random movement, the particles hit each other and also strike the walls of the container. The force exerted by these gas particles per unit area on the walls creates gas pressure.

    ---

    Part 2: The Mystery of Latent Heat

    Have you ever performed this experiment? If you take ice cubes in a beaker, put a thermometer in it, and start heating it over a burner, something surprising happens:

  • The temperature of ice is $0^\circ\text{C}$.
  • As you supply heat, the ice begins to melt.
  • However, the thermometer reading STAYS AT $0^\circ\text{C}$ until ALL the ice has completely melted into water!

    • Where did the heat energy go? Why didn't the temperature rise?

    This hidden heat energy is called Latent Heat (the word *latent* means *hidden*).

    ```

    Heat Supplied ──> Breaks Inter-particle Attractions ──> State Changes (No Temperature Rise)

    ```

    Why does the temperature remain constant during a state change?

    When a substance changes its physical state (solid to liquid, or liquid to gas), the heat energy supplied is absorbed by the particles not to increase kinetic energy (which would raise temperature), but to overcome the strong forces of attraction holding the particles together.

    ---

    1. Latent Heat of Fusion

  • Definition: The amount of heat energy required to change $1\text{ kg}$ of a solid into a liquid at atmospheric pressure at its melting point.
  • Key Concept: Water at $0^\circ\text{C}$ ($273.15\text{ K}$) has more energy than ice at $0^\circ\text{C}$ because the water particles have absorbed the latent heat of fusion.

    • 2. Latent Heat of Vaporization

  • Definition: The amount of heat energy required to change $1\text{ kg}$ of a liquid into gas at atmospheric pressure at its boiling point.
  • Key Concept: Steam at $100^\circ\text{C}$ ($373.15\text{ K}$) has more energy than boiling water at $100^\circ\text{C}$ because steam particles have absorbed the latent heat of vaporization.
    • Crucial Exam Question: Why are burns caused by steam much more severe than burns caused by boiling water at the exact same temperature ($100^\circ\text{C}$)?

    >

    Answer: Steam particles contain extra energy in the form of *latent heat of vaporization*. When steam touches your skin, it releases this additional hidden heat as it condenses into liquid water, resulting in much deeper and more painful burns.

    ---

    Part 3: Evaporation and Factors Affecting It

    We know that water turns into vapor at its boiling point ($100^\circ\text{C}$). But wet clothes dry in the sun, and puddles of water disappear from roads even when the temperature is nowhere near $100^\circ\text{C}$! How?

    This happens through Evaporation.

    What is Evaporation?

    Evaporation is the phenomenon in which a liquid changes into vapor at any temperature below its boiling point.

  • Boiling is a *bulk phenomenon* (happens throughout the entire body of liquid at a fixed temperature).
  • Evaporation is a *surface phenomenon* (particles at the top surface gain enough kinetic energy to break free from liquid attractions).

    • ---

    Factors Affecting the Rate of Evaporation

    There are 4 key factors you must remember for your exams:

    ```

    ┌── Surface Area (Directly proportional ──> ↑ Area = ↑ Evaporation)

    ├── Temperature (Directly proportional ──> ↑ Temp = ↑ Evaporation)

    RATE OF │

    EVAPORATION ─────┼── Humidity (Inversely proportional ──> ↑ Humidity = ↓ Evaporation)

    │

    └── Wind Speed (Directly proportional ──> ↑ Wind = ↑ Evaporation)

    ```

  • Surface Area:
  • Rule: Increasing surface area increases the rate of evaporation.
  • *Real-world example:* We spread out wet clothes on a laundry line to dry them faster instead of leaving them bunched up.
  • Temperature:
  • Rule: Higher temperature increases the rate of evaporation.
  • *Real-world example:* Clothes dry much faster on a hot sunny day than on a cloudy day because more particles get enough kinetic energy to vaporize.
  • Humidity (Amount of water vapor present in air):
  • Rule: Higher humidity decreases the rate of evaporation.
  • *Real-world example:* The air around us can only hold a definite amount of water vapor at a given temperature. On a rainy/monsoon day, the air is already saturated with water, so clothes dry very slowly and we feel sticky.
  • Wind Speed:
  • Rule: Higher wind speed increases the rate of evaporation.
  • *Real-world example:* Clothes dry faster on a windy day because wind blows away water vapor particles from the surroundings, increasing the capacity of surrounding air to take in more vapor.

    • ---

    How Does Evaporation Cause Cooling?

    When a liquid evaporates, the particles at the surface absorb heat energy from the surroundings to regain the energy lost during evaporation. By taking heat away from the surrounding medium, it leaves the surroundings cool!

    Daily Life Examples:

  • Earthen Pots (*Matka*): An earthen pot has millions of tiny microscopic pores. Water continuously seeps through these pores to the outer surface and evaporates. It takes the latent heat of vaporization away from the pot and the remaining water inside, keeping the water cold!
  • Sweating in Summer: Our body produces sweat when it gets hot. As sweat evaporates from our skin surface, it absorbs heat from our body, keeping our internal temperature regulated and cool.
  • Nail Polish Remover / Acetone on Palm: When you pour a drop of acetone or perfume on your palm, it evaporates rapidly. It absorbs energy from your palm, making your palm feel icy cold.
  • Cotton Clothes in Summer: Cotton is a good absorber of water. It absorbs sweat from our body and exposes it to the atmosphere for easy evaporation, providing a cooling effect.

    • ---

    Practice Time! (Questions & Solutions)

    Let me test your understanding! Try answering these questions on your own before reading the detailed solutions.

    ---

    Question 1

    Why does ice at $0^\circ\text{C}$ ($273\text{ K}$) produce a more effective cooling effect in a drink than water at the exact same temperature ($0^\circ\text{C}$)?

    Detailed Solution:

  • Both ice and water can exist at $0^\circ\text{C}$.
  • However, ice at $0^\circ\text{C}$ requires additional energy—specifically the latent heat of fusion—to transform into water at $0^\circ\text{C}$.
  • When ice is placed in a drink, it absorbs heat from the beverage for two purposes:
  • First, to overcome its inter-particle forces of attraction and melt (absorbing latent heat).
  • Second, to raise the temperature of the resulting water.
  • Water at $0^\circ\text{C}$, on the other hand, lacks this extra latent heat capacity and only absorbs heat to raise its own temperature.
  • Therefore, ice absorbs significantly more heat energy from the drink than water does at the same temperature, making ice far more effective at cooling!

    • ---

    Question 2

    During a hot summer afternoon, a student noticed that water droplets form on the outer surface of a tumbler containing ice-cold water. Explain the scientific reason behind this observation.

    Detailed Solution:

  • The phenomenon observed is condensation (the phase change from gas to liquid).
  • Water vapor is naturally present in the surrounding air around the glass.
  • When this airborne water vapor comes into contact with the cold outer surface of the tumbler containing ice-cold water, it loses its kinetic energy (loses heat).
  • As its energy drops, the gas particles slow down and pull closer together, changing state from gaseous water vapor into liquid water droplets.
  • These liquid droplets accumulate and cling to the outer walls of the tumbler.

    • ---

    Question 3

    Give scientific reasons for the following:

  • Tea cools faster when poured into a saucer rather than a teacup.
  • We feel uncomfortable and sweaty on a hot, humid day.

    • Detailed Solution:

  • Saucer vs. Teacup:
  • Evaporation is a surface phenomenon.
  • A saucer has a significantly larger surface area compared to a narrow teacup.
  • A larger surface area allows more surface particles of the hot tea to absorb energy and evaporate simultaneously.
  • Since higher evaporation leads to faster cooling, hot tea cools down much faster in a saucer, making it easier to sip.
  • Hot, Humid Day:
  • Humidity is the amount of moisture/water vapor already present in the air.
  • On a humid day, the air is already saturated with water vapor, which decreases the rate of evaporation.
  • As a result, the sweat produced by our body cannot evaporate easily into the atmosphere.
  • Since sweat doesn't evaporate efficiently, our body loses its natural cooling mechanism, leaving us feeling hot, sticky, and uncomfortable.

    • ---

    Summary Sheet

  • 3 States of Matter: Solids (fixed shape & volume), Liquids (fixed volume, no fixed shape), Gases (no fixed shape or volume).
  • Latent Heat: Hidden heat absorbed or released during a change of state without changing the temperature.
  • Evaporation: Surface phenomenon occurring below boiling point; affected directly by *surface area, temperature, wind speed*, and inversely by *humidity*. Evaporation always leads to cooling.

    • Keep practicing these concepts, revise your NCERT diagrams, and keep asking questions! You are well on your way to acing your Class 9 Science exams!