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Understanding Specific Heat Capacity

4.2 Specific Heat Capacity
PHYSICS • Form 4 • Chapter 4: Heat

4.2 Specific Heat Capacity

In everyday life, different substances heat up or cool down at different rates when exposed to the same amount of heat. For example, at the beach under the hot sun, sand feels very hot quickly while seawater remains cool. This phenomenon is governed by the concepts of heat capacity and specific heat capacity, which describe how much thermal energy is required to produce a given temperature change in an object or substance.

Learning Objectives

  • Define heat capacity, \(C\), and state its SI formula and unit (\(J\ ^\circ C^{-1}\)).
  • Define specific heat capacity, \(c\), and state its formula and SI units (\(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\)).
  • Distinguish between heat capacity and specific heat capacity.
  • Describe laboratory experiments to determine the specific heat capacity of liquids (water) and solids (aluminium).
  • Explain everyday applications and natural phenomena related to specific heat capacity, including cooking utensils, car radiators, building materials, space capsule outer layers, and sea and land breezes.
  • Solve numerical problems involving specific heat capacity using the formula \(Q = mc\Delta\theta\) and conservation of thermal energy (\(Pt = mc\Delta\theta\) and \(Q_1 = Q_2\)).

Comparison of Daily Applications and Natural Phenomena Based on Specific Heat Capacity

Illustrate how substances with low vs. high specific heat capacity behave in heating/cooling, and visualize sea/land breezes alongside cooking utensils and car radiators.

Low Specific Heat Capacity

Gets hot quickly and heats up fast. Examples: metal woks, car engine components, land.

Metal wok Heats up quickly for cooking.
Car engine Transfers heat rapidly.
Land Heats up faster than sea during the day.

High Specific Heat Capacity

Absorbs large heat with small temperature rise. Examples: water, wood, styrofoam, sea.

Water Excellent coolant in car radiators.
Wood Gets hot slowly; used in traditional houses.
Sea Cools down more slowly at night.

Short Explanation

Heat Capacity, \(C\)

Heat capacity is the quantity of heat needed to raise the temperature of the object by \(1\ ^\circ C\).

\(C = \dfrac{Q}{\Delta\theta}\)

Where \(Q\) = quantity of heat supplied (\(J\)) and \(\Delta\theta\) = change in temperature (\(^\circ C\)).

SI unit: \(J\ ^\circ C^{-1}\).

Specific Heat Capacity, \(c\)

Specific heat capacity is the quantity of heat needed to raise the temperature of \(1\ kg\) mass of the substance by \(1\ ^\circ C\).

\(c = \dfrac{Q}{m\Delta\theta}\)

or the heat absorbed/released: \(Q = mc\Delta\theta\)

SI units: \(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\).

Meaning of Value

The specific heat capacity of aluminium is \(900\ J\ kg^{-1}\ ^\circ C^{-1}\). This means \(1\ kg\) of aluminium requires \(900\ J\) of heat to raise its temperature by \(1\ ^\circ C\).

Key Difference

Heat capacity depends on the mass of the object as well as its type of material. Specific heat capacity depends only on the type of material.

SubstanceSpecific Heat Capacity (\(J\ kg^{-1}\ ^\circ C^{-1}\))
Water4 200
Sea water3 900
Ethanol2 500
Paraffin2 100
Olive oil1 890
Cooking oil1 850
Wood1 700
Polycarbonate1 250
Air1 000
Aluminium900
Concrete850
Sand800
Glass670
Iron450
Copper390
Gold300
Mercury140
Lead130

Worked Example: Conservation of Thermal Energy (\(Q_1 = Q_2\))

\(20\text{ g}\) of boiling water at \(100\ ^\circ C\) is poured into a glass containing \(200\text{ g}\) of water at \(28\ ^\circ C\). Calculate the final temperature of the mixture.

Let \(y\) = final temperature of the mixture.

Water that releases heat: \(m_1 = 20\text{ g} = 0.02\text{ kg}\), \(\Delta\theta_1 = (100 - y)\ ^\circ C\)

Water that absorbs heat: \(m_2 = 200\text{ g} = 0.20\text{ kg}\), \(\Delta\theta_2 = (y - 28)\ ^\circ C\)

Specific heat capacity of water, \(c = 4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\).

\(Q_1 = Q_2 \;\Rightarrow\; m_1 c\Delta\theta_1 = m_2 c\Delta\theta_2\)

\(0.02(4\ 200)(100 - y) = 0.20(4\ 200)(y - 28)\)

\(8\ 400 - 84y = 840y - 23\ 520\)

\(924y = 31\ 920\)

\(y = 34.55\ ^\circ C\)

Therefore, the final temperature of the mixture is \(34.55\ ^\circ C\).

Assumption: No heat is absorbed from or released to the surroundings. Heat transfer occurs only between the boiling water and the water at \(28\ ^\circ C\), so the heat released by the boiling water equals the heat absorbed by the water at \(28\ ^\circ C\).

Watch the temperature differences: the body that releases heat gives \((100 - y)\) and the body that absorbs heat gives \((y - 28)\), so both changes stay positive.

Experiments to Determine Specific Heat Capacity

Laboratory methods for water and aluminium.

Experiment 4.1: Water

Wrap the beaker with tissue paper to reduce heat loss. Fill with water until three-quarters full and record mass \(m\). Record initial temperature \(\theta_1\). Turn on the immersion heater and stopwatch simultaneously for \(t = 5\text{ minutes}\) (\(300\ s\)). Switch off the heater and record the highest temperature reading as final temperature \(\theta_2\).

\(c = \dfrac{Pt}{m(\theta_2 - \theta_1)}\)

Experiment 4.2: Aluminium

Wrap a \(1\ kg\) aluminium block with tissue paper. Insert the thermometer and immersion heater into the holes. Put oil in the thermometer hole to ensure better thermal contact. Record initial temperature \(\theta_1\), heat for 5 minutes, switch off the heater, and record the highest temperature \(\theta_2\).

\(c = \dfrac{Pt}{m(\theta_2 - \theta_1)}\)

Applications and Natural Phenomena

Cooking Utensils

Metal woks and pot bodies are made of aluminium or metal with low specific heat capacity so they heat up quickly. Clay pots have high specific heat capacity so food stays hot for a long time. Handles are made of plastic or wood with high specific heat capacity and poor conductivity so they get hot slowly and are safe to hold.

Car Radiator System

Water has a high specific heat capacity, serving as an effective cooling agent. It flows through the engine block to absorb large amounts of heat without boiling, then flows to the radiator where cooling fins and fan airflow release heat quickly.

Traditional Houses and Green Buildings

Traditional houses are built from wood because wood has a high specific heat capacity and gets hot slowly. Green buildings use an insulating concrete roof fitted with styrofoam boards. Styrofoam has a high specific heat capacity, reducing heat absorption from surroundings to lower indoor temperatures.

Space Capsule Outer Layer

Atmospheric friction causes extreme temperatures during reentry. The outer layer is made from materials with high specific heat capacity and high melting points to absorb extreme heat without melting.

Sea Breeze (Daytime)

Land has a lower specific heat capacity than the sea, so land heats up faster. Warm air above land rises; cooler air from the sea moves towards the land.

Land Breeze (Nighttime)

Sea cools down more slowly due to higher specific heat capacity. Warm air above the sea rises; cooler air from land moves towards the sea.

Try to Answer First

Answer in your mind, then press “Check Answer”.

1

What is the difference between heat capacity and specific heat capacity?

Check Answer
Answer: Heat capacity is the heat energy required to raise the temperature of an entire object by \(1\ ^\circ C\) (\(C = \frac{Q}{\Delta\theta}\)), whereas specific heat capacity is the heat energy required to raise the temperature of \(1\ kg\) of a substance by \(1\ ^\circ C\) (\(c = \frac{Q}{m\Delta\theta}\)).
2

How much heat energy is needed to increase the temperature of a \(0.2\ kg\) mass of gold by \(10\ ^\circ C\)? (Given \(c_{\text{gold}} = 300\ J\ kg^{-1}\ ^\circ C^{-1}\))

Check Answer
Answer: \(Q = mc\Delta\theta = (0.2\ kg) \times (300\ J\ kg^{-1}\ ^\circ C^{-1}) \times (10\ ^\circ C) = 600\ J\).
3

Why is water used as the cooling fluid in a car radiator system?

Check Answer
Answer: Water has a very high specific heat capacity (\(4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\)), which enables it to absorb a large amount of heat from the engine block with only a small increase in its own temperature.

Common Mistakes

  • !Confusing heat capacity (\(C\)) with specific heat capacity (\(c\)), leading to incorrect units (\(J\ ^\circ C^{-1}\) vs \(J\ kg^{-1}\ ^\circ C^{-1}\)).
  • !Forgetting to convert mass into kilograms (\(kg\)) when calculating using \(Q = mc\Delta\theta\) (e.g., using grams directly).
  • !Forgetting to convert heating time from minutes into seconds (\(s\)) when calculating energy from heater power (\(Q = Pt\)).
  • !Writing the temperature difference incorrectly in thermal exchange problems (e.g., writing \((28 - y)\) instead of \((y - 28)\) for the substance absorbing heat).
  • !Assuming experimental values of \(c\) will perfectly equal theoretical values, ignoring heat loss to surroundings or heat absorbed by the container.

Concept Misunderstandings

Misunderstanding

A substance with a high specific heat capacity gets hot faster because it holds more heat.

Correct Concept

A high specific heat capacity means the substance needs a large amount of heat to produce even a small temperature rise, so it heats up more slowly than a substance with low specific heat capacity.

Misunderstanding

Heat capacity depends only on the material of the object.

Correct Concept

Heat capacity (\(C\)) depends on both the type of material and the total mass of the object. Specific heat capacity (\(c\)) depends only on the type of material.

Misunderstanding

The final temperature of water in the experiment should be recorded the instant the heater is switched off.

Correct Concept

Heat continues to conduct from the immersion heater into the water for a brief period; hence, the highest temperature reading observed on the thermometer after switching off must be recorded.

Summary

  • Heat capacity (\(C = \frac{Q}{\Delta\theta}\), unit: \(J\ ^\circ C^{-1}\)) depends on mass and material.
  • Specific heat capacity (\(c = \frac{Q}{m\Delta\theta}\), unit: \(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\)) is an intrinsic property of a substance.
  • The thermal energy formula is \(Q = mc\Delta\theta\), and for electrical heating, \(Pt = mc\Delta\theta\).
  • Water has a remarkably high specific heat capacity (\(4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\)), making it ideal for car cooling radiators and causing daytime sea breezes and nighttime land breezes.
  • Metals have low specific heat capacities, enabling them to heat up and transfer heat quickly.

Short Activity

Objective: Test your understanding of heat capacity, specific heat capacity and their applications.

A. Objective Quiz

1 Which statement correctly explains why sand on a beach gets hotter much faster than seawater during the day?

2 An electric heater of power \(50\ W\) heats a \(0.5\ kg\) metal block for \(90\ s\). If the temperature rises by \(25\ ^\circ C\) and no heat is lost, what is the specific heat capacity of the metal?

B. Fill in the Blanks

3 The quantity of heat needed to raise the temperature of \(1\ kg\) mass of a substance by \(1\ ^\circ C\) is known as its .

4 The SI unit for heat capacity (\(C\)) is .

C. Matching / Drag and Drop

Match each application or feature to the correct role or reason based on specific heat capacity. If using a phone, tap the answer first, then tap the matching box.

Application / Material
Aluminium pot body
Plastic pot handle
Water in car radiator
Sea breeze during daytime
Functional Reason
Low specific heat capacity to heat up quickly for cookingCorrect ✓Try againEmpty
High specific heat capacity so it gets hot slowly and is safe to holdCorrect ✓Try againEmpty
High specific heat capacity to absorb large amounts of heat as a cooling agentCorrect ✓Try againEmpty
Land heats up faster than sea, causing warm air over land to rise and cool air from sea to move inCorrect ✓Try againEmpty
 

Keywords

Heat capacity (\(C\)) Specific heat capacity (\(c\)) Cooling agent Sea breeze Land breeze Thermal contact
The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.

Understanding Specific Heat Capacity

4.2 Specific Heat Capacity
PHYSICS • Form 4 • Chapter 4: Heat

4.2 Specific Heat Capacity

In everyday life, different substances heat up or cool down at different rates when exposed to the same amount of heat. For example, at the beach under the hot sun, sand feels very hot quickly while seawater remains cool. This phenomenon is governed by the concepts of heat capacity and specific heat capacity, which describe how much thermal energy is required to produce a given temperature change in an object or substance.

Learning Objectives

  • Define heat capacity, \(C\), and state its SI formula and unit (\(J\ ^\circ C^{-1}\)).
  • Define specific heat capacity, \(c\), and state its formula and SI units (\(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\)).
  • Distinguish between heat capacity and specific heat capacity.
  • Describe laboratory experiments to determine the specific heat capacity of liquids (water) and solids (aluminium).
  • Explain everyday applications and natural phenomena related to specific heat capacity, including cooking utensils, car radiators, building materials, space capsule outer layers, and sea and land breezes.
  • Solve numerical problems involving specific heat capacity using the formula \(Q = mc\Delta\theta\) and conservation of thermal energy (\(Pt = mc\Delta\theta\) and \(Q_1 = Q_2\)).

Comparison of Daily Applications and Natural Phenomena Based on Specific Heat Capacity

Illustrate how substances with low vs. high specific heat capacity behave in heating/cooling, and visualize sea/land breezes alongside cooking utensils and car radiators.

Low Specific Heat Capacity

Gets hot quickly and heats up fast. Examples: metal woks, car engine components, land.

Metal wok Heats up quickly for cooking.
Car engine Transfers heat rapidly.
Land Heats up faster than sea during the day.

High Specific Heat Capacity

Absorbs large heat with small temperature rise. Examples: water, wood, styrofoam, sea.

Water Excellent coolant in car radiators.
Wood Gets hot slowly; used in traditional houses.
Sea Cools down more slowly at night.

Short Explanation

Heat Capacity, \(C\)

Heat capacity is the quantity of heat needed to raise the temperature of the object by \(1\ ^\circ C\).

\(C = \dfrac{Q}{\Delta\theta}\)

Where \(Q\) = quantity of heat supplied (\(J\)) and \(\Delta\theta\) = change in temperature (\(^\circ C\)).

SI unit: \(J\ ^\circ C^{-1}\).

Specific Heat Capacity, \(c\)

Specific heat capacity is the quantity of heat needed to raise the temperature of \(1\ kg\) mass of the substance by \(1\ ^\circ C\).

\(c = \dfrac{Q}{m\Delta\theta}\)

or the heat absorbed/released: \(Q = mc\Delta\theta\)

SI units: \(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\).

Meaning of Value

The specific heat capacity of aluminium is \(900\ J\ kg^{-1}\ ^\circ C^{-1}\). This means \(1\ kg\) of aluminium requires \(900\ J\) of heat to raise its temperature by \(1\ ^\circ C\).

Key Difference

Heat capacity depends on the mass of the object as well as its type of material. Specific heat capacity depends only on the type of material.

SubstanceSpecific Heat Capacity (\(J\ kg^{-1}\ ^\circ C^{-1}\))
Water4 200
Sea water3 900
Ethanol2 500
Paraffin2 100
Olive oil1 890
Cooking oil1 850
Wood1 700
Polycarbonate1 250
Air1 000
Aluminium900
Concrete850
Sand800
Glass670
Iron450
Copper390
Gold300
Mercury140
Lead130

Worked Example: Conservation of Thermal Energy (\(Q_1 = Q_2\))

\(20\text{ g}\) of boiling water at \(100\ ^\circ C\) is poured into a glass containing \(200\text{ g}\) of water at \(28\ ^\circ C\). Calculate the final temperature of the mixture.

Let \(y\) = final temperature of the mixture.

Water that releases heat: \(m_1 = 20\text{ g} = 0.02\text{ kg}\), \(\Delta\theta_1 = (100 - y)\ ^\circ C\)

Water that absorbs heat: \(m_2 = 200\text{ g} = 0.20\text{ kg}\), \(\Delta\theta_2 = (y - 28)\ ^\circ C\)

Specific heat capacity of water, \(c = 4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\).

\(Q_1 = Q_2 \;\Rightarrow\; m_1 c\Delta\theta_1 = m_2 c\Delta\theta_2\)

\(0.02(4\ 200)(100 - y) = 0.20(4\ 200)(y - 28)\)

\(8\ 400 - 84y = 840y - 23\ 520\)

\(924y = 31\ 920\)

\(y = 34.55\ ^\circ C\)

Therefore, the final temperature of the mixture is \(34.55\ ^\circ C\).

Assumption: No heat is absorbed from or released to the surroundings. Heat transfer occurs only between the boiling water and the water at \(28\ ^\circ C\), so the heat released by the boiling water equals the heat absorbed by the water at \(28\ ^\circ C\).

Watch the temperature differences: the body that releases heat gives \((100 - y)\) and the body that absorbs heat gives \((y - 28)\), so both changes stay positive.

Experiments to Determine Specific Heat Capacity

Laboratory methods for water and aluminium.

Experiment 4.1: Water

Wrap the beaker with tissue paper to reduce heat loss. Fill with water until three-quarters full and record mass \(m\). Record initial temperature \(\theta_1\). Turn on the immersion heater and stopwatch simultaneously for \(t = 5\text{ minutes}\) (\(300\ s\)). Switch off the heater and record the highest temperature reading as final temperature \(\theta_2\).

\(c = \dfrac{Pt}{m(\theta_2 - \theta_1)}\)

Experiment 4.2: Aluminium

Wrap a \(1\ kg\) aluminium block with tissue paper. Insert the thermometer and immersion heater into the holes. Put oil in the thermometer hole to ensure better thermal contact. Record initial temperature \(\theta_1\), heat for 5 minutes, switch off the heater, and record the highest temperature \(\theta_2\).

\(c = \dfrac{Pt}{m(\theta_2 - \theta_1)}\)

Applications and Natural Phenomena

Cooking Utensils

Metal woks and pot bodies are made of aluminium or metal with low specific heat capacity so they heat up quickly. Clay pots have high specific heat capacity so food stays hot for a long time. Handles are made of plastic or wood with high specific heat capacity and poor conductivity so they get hot slowly and are safe to hold.

Car Radiator System

Water has a high specific heat capacity, serving as an effective cooling agent. It flows through the engine block to absorb large amounts of heat without boiling, then flows to the radiator where cooling fins and fan airflow release heat quickly.

Traditional Houses and Green Buildings

Traditional houses are built from wood because wood has a high specific heat capacity and gets hot slowly. Green buildings use an insulating concrete roof fitted with styrofoam boards. Styrofoam has a high specific heat capacity, reducing heat absorption from surroundings to lower indoor temperatures.

Space Capsule Outer Layer

Atmospheric friction causes extreme temperatures during reentry. The outer layer is made from materials with high specific heat capacity and high melting points to absorb extreme heat without melting.

Sea Breeze (Daytime)

Land has a lower specific heat capacity than the sea, so land heats up faster. Warm air above land rises; cooler air from the sea moves towards the land.

Land Breeze (Nighttime)

Sea cools down more slowly due to higher specific heat capacity. Warm air above the sea rises; cooler air from land moves towards the sea.

Try to Answer First

Answer in your mind, then press “Check Answer”.

1

What is the difference between heat capacity and specific heat capacity?

Check Answer
Answer: Heat capacity is the heat energy required to raise the temperature of an entire object by \(1\ ^\circ C\) (\(C = \frac{Q}{\Delta\theta}\)), whereas specific heat capacity is the heat energy required to raise the temperature of \(1\ kg\) of a substance by \(1\ ^\circ C\) (\(c = \frac{Q}{m\Delta\theta}\)).
2

How much heat energy is needed to increase the temperature of a \(0.2\ kg\) mass of gold by \(10\ ^\circ C\)? (Given \(c_{\text{gold}} = 300\ J\ kg^{-1}\ ^\circ C^{-1}\))

Check Answer
Answer: \(Q = mc\Delta\theta = (0.2\ kg) \times (300\ J\ kg^{-1}\ ^\circ C^{-1}) \times (10\ ^\circ C) = 600\ J\).
3

Why is water used as the cooling fluid in a car radiator system?

Check Answer
Answer: Water has a very high specific heat capacity (\(4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\)), which enables it to absorb a large amount of heat from the engine block with only a small increase in its own temperature.

Common Mistakes

  • !Confusing heat capacity (\(C\)) with specific heat capacity (\(c\)), leading to incorrect units (\(J\ ^\circ C^{-1}\) vs \(J\ kg^{-1}\ ^\circ C^{-1}\)).
  • !Forgetting to convert mass into kilograms (\(kg\)) when calculating using \(Q = mc\Delta\theta\) (e.g., using grams directly).
  • !Forgetting to convert heating time from minutes into seconds (\(s\)) when calculating energy from heater power (\(Q = Pt\)).
  • !Writing the temperature difference incorrectly in thermal exchange problems (e.g., writing \((28 - y)\) instead of \((y - 28)\) for the substance absorbing heat).
  • !Assuming experimental values of \(c\) will perfectly equal theoretical values, ignoring heat loss to surroundings or heat absorbed by the container.

Concept Misunderstandings

Misunderstanding

A substance with a high specific heat capacity gets hot faster because it holds more heat.

Correct Concept

A high specific heat capacity means the substance needs a large amount of heat to produce even a small temperature rise, so it heats up more slowly than a substance with low specific heat capacity.

Misunderstanding

Heat capacity depends only on the material of the object.

Correct Concept

Heat capacity (\(C\)) depends on both the type of material and the total mass of the object. Specific heat capacity (\(c\)) depends only on the type of material.

Misunderstanding

The final temperature of water in the experiment should be recorded the instant the heater is switched off.

Correct Concept

Heat continues to conduct from the immersion heater into the water for a brief period; hence, the highest temperature reading observed on the thermometer after switching off must be recorded.

Summary

  • Heat capacity (\(C = \frac{Q}{\Delta\theta}\), unit: \(J\ ^\circ C^{-1}\)) depends on mass and material.
  • Specific heat capacity (\(c = \frac{Q}{m\Delta\theta}\), unit: \(J\ kg^{-1}\ ^\circ C^{-1}\) or \(J\ kg^{-1}\ K^{-1}\)) is an intrinsic property of a substance.
  • The thermal energy formula is \(Q = mc\Delta\theta\), and for electrical heating, \(Pt = mc\Delta\theta\).
  • Water has a remarkably high specific heat capacity (\(4\ 200\ J\ kg^{-1}\ ^\circ C^{-1}\)), making it ideal for car cooling radiators and causing daytime sea breezes and nighttime land breezes.
  • Metals have low specific heat capacities, enabling them to heat up and transfer heat quickly.

Short Activity

Objective: Test your understanding of heat capacity, specific heat capacity and their applications.

A. Objective Quiz

1 Which statement correctly explains why sand on a beach gets hotter much faster than seawater during the day?

2 An electric heater of power \(50\ W\) heats a \(0.5\ kg\) metal block for \(90\ s\). If the temperature rises by \(25\ ^\circ C\) and no heat is lost, what is the specific heat capacity of the metal?

B. Fill in the Blanks

3 The quantity of heat needed to raise the temperature of \(1\ kg\) mass of a substance by \(1\ ^\circ C\) is known as its .

4 The SI unit for heat capacity (\(C\)) is .

C. Matching / Drag and Drop

Match each application or feature to the correct role or reason based on specific heat capacity. If using a phone, tap the answer first, then tap the matching box.

Application / Material
Aluminium pot body
Plastic pot handle
Water in car radiator
Sea breeze during daytime
Functional Reason
Low specific heat capacity to heat up quickly for cookingCorrect ✓Try againEmpty
High specific heat capacity so it gets hot slowly and is safe to holdCorrect ✓Try againEmpty
High specific heat capacity to absorb large amounts of heat as a cooling agentCorrect ✓Try againEmpty
Land heats up faster than sea, causing warm air over land to rise and cool air from sea to move inCorrect ✓Try againEmpty
 

Keywords

Heat capacity (\(C\)) Specific heat capacity (\(c\)) Cooling agent Sea breeze Land breeze Thermal contact
The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.
Chapter : Heat
Topic : Specific Heat Capacity
Form 4 Physics
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