Grade 10
  1. Mechanics  1.1. Dynamics  1.1.1. Motion in one dimension  1.1.2. Motion in two dimensions  1.1.3. Displacement and Distance  1.1.4. Speed and Velocity  1.1.5. Acceleration  1.1.6. Graphical representation of motion  1.1.7. Equations of motion  1.1.8. Free fall and acceleration due to gravity  1.1.9. Projectile motion  1.1.10. Relative speed  1.2. Dynamics  1.2.1. Newton's Laws of Motion  1.2.2. Inertia and mass  1.2.3. Force and its types  1.2.4. action and reaction force  1.2.5. Friction and its effects  1.2.6. Coefficient of friction  1.2.7. Circular motion  1.2.8. Centripetal force and centripetal acceleration  1.2.9. Momentum and Impulse  1.2.10. Conservation of momentum  1.2.11. Newton's third law and applications  1.3. Work, Energy and Power  1.3.1. Work done by the force  1.3.2. Work–energy theorem  1.3.3. Kinetic energy  1.3.4. Potential energy  1.3.5. Mechanical energy  1.3.6. Energy Conservation  1.3.7. Power and efficiency  1.3.8. Renewable and non-renewable energy sources  1.4. Gravitational force  1.4.1. Newton's law of universal gravitation  1.4.2. Gravitational field and field strength  1.4.3. Acceleration due to gravity on different planets  1.4.4. Kepler's laws of planetary motion  1.4.5. Orbits and satellites  1.4.6. Weight and apparent weight  1.4.7. Gravitational potential energy
  2. Properties of matter  2.1. States of matter  2.1.1. Solid, liquid and gas  2.1.2. Molecular structure of matter  2.1.3. Intermolecular forces  2.1.4. Plasma and Bose–Einstein condensate  2.2. Pressure  2.2.1. Definition of Pressure  2.2.2. Pressure in liquids  2.2.3. Atmospheric pressure  2.2.4. Pascal's principle  2.2.5. Archimedes' Principle and Buoyancy  2.2.6. Surface tension and capillarity  2.3. Elasticity  2.3.1. Hooke's law  2.3.2. Stress and strain  2.3.3. Elastic Limit and Modulus of Elasticity  2.3.4. Applications of Elasticity
  3. Thermal physics  3.1. heat and temperature  3.1.1. Difference Between Heat and Temperature  3.1.2. Temperature scale  3.1.3. Thermal expansion  3.1.4. Thermal equilibrium  3.2. Heat transfer  3.2.1. Conductivity  3.2.2. Convection  3.2.3. Radiation  3.2.4. Insulation and its applications  3.3. Thermal properties of matter  3.3.1. Specific heat capacity  3.3.2. Latent heat and phase change  3.3.3. Boiling and Melting Point  3.3.4. Heat engines and refrigeration  3.4. Laws of Thermodynamics  3.4.1. Zeroth law of thermodynamics  3.4.2. First law of thermodynamics  3.4.3. Second law of thermodynamics  3.4.4. Carnot cycle
  4. Waves and optics  4.1. Nature and properties of waves  4.1.1. Types of waves in nature and properties of waves  4.1.2. Transverse and longitudinal waves  4.1.3. Wave parameters  4.1.4. Reflection and refraction of waves  4.1.5. Superposition and Interference  4.1.6. Standing Waves and Resonance  4.1.7. Doppler effect  4.2. Sound waves  4.2.1. Characteristics of sound waves  4.2.2. Speed of sound in different mediums  4.2.3. Applications of sound waves  4.2.4. Ultrasound and its uses  4.3. Light Waves and Optics  4.3.1. Nature of light  4.3.2. Reflection of light  4.3.3. Laws of reflection  4.3.4. Mirrors and Image Formation  4.3.5. Refraction of light  4.3.6. Snell's Law  4.3.7. Lenses and Image Formation  4.3.8. Total internal reflection and critical angle  4.3.9. Optical fibre  4.4. Optical Instruments  4.4.1. Microscope  4.4.2. Telescope  4.4.3. Human eye and vision defects  4.4.4. Camera and its working principle
  5. Electricity and Magnetism  5.1. Electrostatics  5.1.1. Electric charge and its properties  5.1.2. Conductors and Insulators  5.1.3. Coulomb's law  5.1.4. Electric field and field lines  5.1.5. Electric potential and potential difference  5.1.6. Capacitors and Capacitance  5.2. Current Electricity  5.2.1. Electric current and its measurement  5.2.2. Ohm's law  5.2.3. Resistance and resistivity  5.2.4. Series and Parallel Circuits  5.2.5. Electric power and energy  5.2.6. Kirchhoff's Laws  5.3. Magnetism and Electromagnetism  5.3.1. Magnetic field and field lines  5.3.2. Magnetic effects of electric current  5.3.3. Electromagnetic induction  5.3.4. Faraday's laws of electromagnetic induction  5.3.5. Transformers and Applications  5.3.6. AC and DC current
  6. Modern Physics  6.1. Nuclear physics  6.1.1. Structure of the atom  6.1.2. Bohr's atomic model  6.1.3. Electron Energy Levels  6.1.4. X-rays and applications  6.2. Radioactivity  6.2.1. Types of radiation  6.2.2. Half-life and radioactive decay  6.2.3. Nuclear reactions and applications  6.2.4. Fission and Fusion  6.3. Quantum physics  6.3.1. Wave–particle duality  6.3.2. Photoelectric effect  6.3.3. Energy quantization  6.3.4. Heisenberg's uncertainty principle
  7. Electronics and Communication  7.1. Semiconductors  7.1.1. Conductors, Insulators and Semiconductors  7.1.2. Diodes and their applications  7.1.3. Transistors and Logic Gates  7.1.4. LEDs and photodiodes  7.2. Communication Systems  7.2.1. Basics of communication  7.2.2. Analog and digital signals  7.2.3. Wireless and optical fibre communication  7.2.4. Radio Waves and Modulation

Grade 10 → Thermal physics → Thermal properties of matter ↓


Specific heat capacity


The concept of specific heat capacity is crucial to understanding how substances behave when they are heated or cooled. This property of matter is a fundamental concept in the field of thermal physics and is important in a wide range of applications, from industrial processes to everyday phenomena. In this detailed document, we will explore every aspect of specific heat capacity, delve deeper into its implications and examine practical examples to build a comprehensive understanding.

What is heat?

Before diving into specific heat capacity, it's important to understand what heat is. Heat is a form of energy transfer between a system and its surroundings due to a temperature difference. When you heat an object, its temperature increases, which means the molecules inside it begin to move faster. This molecular motion is a manifestation of energy.

Defining specific heat capacity

Specific heat capacity is defined as the amount of heat required to raise the temperature of one kilogram of a substance by one degree Celsius (°C) or one Kelvin (K). This is a property that varies from substance to substance.

The formula to calculate the heat energy (q) required is:

q = mcΔT
  • q is the thermal energy in joules (J).
  • m is the mass of the object in kilograms (kg).
  • c is the specific heat capacity (joules per kilogram per degree Celsius).
  • ΔT is the change in temperature in degrees Celsius (°C) or Kelvin (K).

Example: Calculating heat energy

Imagine that you have a 2 kg piece of iron, and you need to calculate the energy needed to raise its temperature by 10°C. Assuming that the specific heat capacity of iron is c 450 J/kg°C, you can use the formula:

q = mcΔT
q = 2 kg × 450 J/kg°C × 10°C = 9000 J

You will need 9000 joules of energy to achieve the desired temperature rise for the piece of iron.

Visualizing specific heat capacity

Material A high specific heat Material B low specific heat

In the visualization above, both material A and material B absorb the same amount of heat. However, due to the different specific heat capacities, material A has a smaller change in temperature, indicating a higher specific heat capacity, while material B has a greater temperature increase, indicating a lower specific heat capacity.

Factors affecting specific heat capacity

The specific heat capacity of a substance depends on many factors, such as its molecular structure and the state it is in (solid, liquid, or gas). Here are some of the key factors:

  • Molecular structure: Substances with complex molecules often have higher specific heat capacities because they have more ways to store energy.
  • Bonding: Substances with strong bonds generally have low specific heat capacities because energy is used to break these bonds rather than to increase molecular motion.
  • State of matter: Gases generally have the highest specific heat capacity, followed by liquids, and then solids.

Applications of specific heat capacity

Specific heat capacity has a wide range of uses in everyday life and in various industries. Here are some examples:

  • Climate and weather: Water's high specific heat capacity plays an important role in regulating the Earth's climate, as it absorbs and releases heat over time.
  • Cooking: Different cooking vessels are made of materials with different specific heat capacities, which affects how quickly they heat up or cool down.
  • Engineering: Specific heat capacity is important in designing heating and cooling systems such as radiators and heat exchangers.

Example: Cooking with specific heat capacity

If you use a cast iron skillet (c ≈ 450 J/kg°C), compared to an aluminum skillet (c ≈ 900 J/kg°C), cast iron will take longer to heat up, but it will also retain heat longer. The choice of skillet material can affect cooking times and the texture of food.

Measuring specific heat capacity

Specific heat capacity can be measured experimentally, by determining how much heat a known mass of a substance absorbs to change its temperature by a certain amount. A frequently used method is calorimetry:

  1. Heat a substance of known mass.
  2. Measure temperature changes.
  3. Use a calorimeter to ensure minimum heat loss to the surrounding environment.

Example: Calorimetry

In an experiment, a 100 g piece of metal is heated to 100°C and then immersed in a calorimeter containing 150 g of water initially at 25°C. If the final water temperature is 30°C, the specific heat of the metal can be calculated using the formula, with the heat capacity of water being 4.18 J/g°C.

heat gained by water = heat lost by metal
(m × c × ΔT)_{water} = (m × c × ΔT)_{metal}

Further exploration: Difference between specific heat capacity and heat capacity

It is easy to confuse specific heat capacity and heat capacity. However, they refer to slightly different concepts.

  • Heat capacity: It is the amount of heat required to raise the temperature of an object by one degree Celsius, regardless of its mass. It depends on the substance and mass.
  • Specific heat capacity: As already defined, it is the heat required to raise the temperature of a unit mass of a substance by one degree Celsius and it does not depend on mass.

Specific heat capacity in everyday life

Understanding specific heat capacity can increase our understanding of everyday phenomena and improve our decision-making about the use of materials. Here are some more examples:

  • Automobile engines: Coolants used in engines have a high specific heat capacity, allowing them to effectively absorb and dissipate heat, improving performance and safety.
  • Construction materials: Materials such as concrete have a high specific heat capacity, making them suitable for thermal mass in construction, as they help regulate temperature fluctuations.
  • Thermal insulation: Insulators with low specific heat capacity are selected to resist heating or cooling, providing comfort and energy efficiency.

Conclusion

Specific heat capacity is a powerful concept that helps us understand and manipulate how substances exchange heat. Different substances react to heat in different ways because of their specific heat capacity, affecting everything from cooking utensils to climate systems. By recognizing the importance of this thermal property, we can make more informed choices in engineering, everyday applications, and scientific studies.


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Specific heat capacity

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