Samacheer Kalvi 9th Science Solutions Chapter 7 Heat

Samacheer Kalvi 9th Science Solutions Chapter 7 Heat

Samacheer Kalvi 9th Science Heat Textbook Exercises

Question 1.
Calorie is the unit of
(a) heat
(b) work
(c) temperature
(d) food
(a) heat

Question 2.
SI unit of temperature is
(a) fahrenheit
(b) joule
(c) Celsius
(d) kelvin
(d) kelvin

Question 3.
Two cylindrical rods of same length have the area of cross-section in the ratio 2:1. If both the rods are made up of same material, which of them conduct heat faster?
(a) Both rods
(b) Rod-2
(c) Rod-1
(d) None of them
(c) Rod-1

Question 4.
In which mode of transfer of heat, molecules pass on heat energy to neighbouring molecules without actually moving from their positions?
(b) Conduction
(c) Convection
(d) Both B and C
(b) Conduction

Question 5.
A device in which the loss of heat due to conduction, convection and radiation is minimized is
(a) Solar cell
(b) Solar cooker
(c) Thermometer

1.  (a) Heat
2.  (d) kelvin
3.  (c) Rod-1
4.  (b) Conduction

II. Fill in the blanks.

1. The fastest mode of heat transfer is ……………….
2. During day time, air blows from ………… to …………….
3. Liquids and gases are generally …………….. conductors of heat.
4. The fixed temperature at which matter changes state from solid to liquid is called ………………

2. land, sea
4. melting point

III. Assertion and Reason type questions.

Mark the correct choice as:
(a) If both assertion and reason are true and reason is the correct explanation of assertion.
(b) If both assertion and reason are true but reason is not the correct explanation of assertion.
(c) If assertion is true but reason is false.
(d) If assertion is false but reason is true.

Question 1.
Assertion(A): Food can be cooked faster in copper bottom vessels.
Reason (R): Copper is the best conductor of heat.
(a) If both assertion and reason are true and reason is the correct explanation of assertion.

Question 2.
Assertion(A): Maximum sunlight reaches earth’s surface during the afternoon time.
Reason(R): Heat from the sun reaches earth’s surface by radiation.
(b) If both assertion and reason are true but reason is not the correct explanation of assertion.

Question 3.
Assertion(A): When water is heated up to 100°C, there is no raise in temperature until all water gets converted into water vapour.

Reason(R): Boiling point of water is 10°C.
(c) If assertion is true but reason is false.

Question 1.
Define conduction.
The process of transfer of heat in solids from a region of higher temperature to a region of lower temperature without the actual movement of molecules is called conduction.

Question 2.
Ice is kept in a double-walled container. Why?
Ice is kept in a double-walled container so as to prevent melting of ice from the heat absorbed present in the immediate surroundings. The vacuum present in between the two walls prevents the transfer of heat from the first to the second wall and hence the ice remains in the solid form for a longer time period.

Question 3.
How does the water keep in an earthen pot remain cool?
As the water seeps out of the earthen pot, it gets evaporated and takes away heat from the vessel. The water in the pot §ets cooled.

Question 4.

 S.No. Convection Radiation 1. Flow of heat through a fluid from places of higher temperature to places of lower temperature by movement of the fluid itself. Flow of heat from one place to another by means of electromagnetic waves. 2. Convection needs matter to be present. Radiation can occur even in vacuum. 3. Convection seen in daily life: Hot air balloons, breeze, wind, chimney. Radiation in daily life: White or light coloured cloths, highly polished surface of airplane, helps to reflect most of the heat radiation from the sun.

Question 5.
Why do people prefer wearing white clothes during summer?
White clothes absorb the least heat from the sun and hence keep us comfortable in summer. On the other hand, dark coloured clothes absorb more heat from the sun and keep us warm in winter.

Question 6.
What is specific heat capacity?

• The specific heat capacity of a substance is defined as the amount of heat required to raise the temperature of 1 kg of the substance by 1°C or 1 K.
• Q = mC∆T, where Q is the quantity of heat required to raise the temperature and m is the mass of the body and AT is the change in temperature of the body.
• The SI unit of specific heat capacity is Jkg– 1 K– 1. The most commonly used units of specific heat capacity are J/kg°C and J/g°C.

Question 7.
Define thermal capacity.
Thermal capacity is the heat required to raise the temperature of a unit mass of the body by 1°C.

Question 8.
Define specific latent heat capacity.

• Specific latent heat is the amount of heat energy absorbed or liberated by unit mass of a substance during change of state without causing any change in temperature.
• Specific latent heat is given as L = Q/m, where ‘Q’ is the amount of heat energy absorbed or liberated and ‘m’ is mass of a substance during its change of phase at a constant temperature.
• The SI unit of specific latent heat is J/kg.

Question 1.
Explain convection in daily life.
Convection in daily life:
(i) Hot air balloons: Air molecules at the bottom of the balloon get heated by a heat source and rise. As the warm air rises, cold air is pushed downward and it is also heated. When the hot air is trapped inside the balloon, it rises.

(ii) Breeze: During day time, the air in contact with the land becomes hot and rises. Now the cool air over the surface of the sea replaces it. It is called sea breeze. During nighttime, air above the sea is warmer. As the warmer air over the surface of the sea rises, cooler air above the land moves towards the sea.

(iii) Winds: Air flows from area of high pressure to area of low pressure. The warm air molecules over the hot surface rise and create low pressure. So, cooler air with high pressure flows towards the low-pressure area. This causes wind flow.
(iv) Chimneys: Tall chimneys are kept in the kitchen and industrial furnaces. As the hot gases and smoke are lighter, they rise up in the atmosphere.

Question 2.
What are the changes of state in the water? Explain.
Any matter around us can be in three forms: solid, liquid and gas, called states of matter. Depending upon the temperature, pressure and transfer of heat, matter is converted from one state to another and is known as change of state in matter. There are different such processes in the change of state in matter.

For example;

• Water molecules are in liquid state at normal temperature. When water is heated to 100°C, it becomes steam or vapour which is a gaseous state of matter. The process by which a
liquid is converted to vapour by absorbing heat is called boiling or vaporization.
• The temperature at which a liquid changes its state to gas is called boiling point.
• On reducing the temperature of the steam it becomes water again. The process by which a vapour is converted to liquid by releasing heat is called condensation. On reducing the temperature of water further to 0°C, it becomes ice which is a solid state of water.
• The process by which a liquid is converted to solid by releasing heat is called freezing. The
temperature by which a liquid changes its state to solid is called freezing point. Ice on
heating, becomes water again by absorbing heat, a process known as melting.
• Dry ice changes directly to gaseous state without becoming liquid. This process is called
sublimation.

Thus, water changes its state when there is a change in temperature.

Question 3.
How can you experimentally prove that water is a bad conductor of heat? How is it possible to heat water easily while cooking.
Experiment to prove that water is a bad conductor of heat:
Take a glass tube and drop an ice cube wrapped in wire gauze in it.
Now fill 3/4th of this tube with water and place it above the burner as shown in the figure.
You can observe that the water boils at the edge and the ice present in the bottom of the tube has not melted indicating that heat has not reached the bottom where the ice cube is present. This proves that water is a bad conductor of heat.
It is easy to heat water easily or quickly while cooking. This is because, while cooking the vessel or pan is usually covered with a lid.

1. Radiation from the hot water is reflected back into the pan rather than being emitted
2. Free convection is effectively eliminated, and
3. Evaporative cooling’ is also eliminated.
This in turn allows the water to be heated more easily.

VI. Problems:

Question 1.
What is the heat in joules required to raise the temperature of 25 grams of water from 0°C to 100°C? What is the heat in Calories? (Specific heat of water = 4.18 J/g°C).
Solution:
Given m = 25 g, ∆T = (100 – 0) = 100°C
Or in terms of Kelvin (373.15 – 273.15) = 100K,
C = 4.18J/g°C
Heat energy required, Q = m × C × ∆T = 25 × 4.18 × 100 = 10450 J

Question 2.
What could be the final temperature of a mixture of 100 g of water at 90°C and 600g of water at 20°C.
Solution:
To find final temperature: ∆Q = mc
lOOg of water originally at 90°C will loose an amount of heat,
∆Q = mc ∆T
∆Q = 100 × c × (90 – T)
The same amount of heat will be absorbed by 600g of water originally at 20°C to raise its temperature to T.
∆Q = 600 × c × (T – 30)
⇒ 600C (T – 20°) = 100C (90° – T)
⇒ 6T – 120° = 90° – T
⇒ 6T + T = 120° + 90°
⇒ 7T = 210°
⇒ T = 210/7
⇒ T = 30°C

Question 3.
How much heat energy is required to change 2 kg of ice at 0°C into the water at 20°C? (Specific latent heat of fusion of water = 3,34,000J/kg, Specific heat capacity of water = 4200Jkg– 1 K– 1 ).
Solution:
Total heat = Heat required to convert 2Kg of ice into water at 0°C + Heat required to convert 2Kg of water at 0°C to 2Kg of water at 20°C
Heat = m (hfw) + mc∆T
Here, m(mass of ice) = 2Kg
hfw (specific latent heat of water) = 3,34,000J/Kg
C (specific heat capacity of water) = 4200JKg– 1K– 1
AT (Temperature difference) = 20°C
Therefore, Heat required = (2 × 334000) + (2 × 4200) (20 – 0)
= 668000 + 8400 (20)
= 668000+ 168000
Heat required = 8,36,000 J

Activity

Question 1.
Take a glass of water and put some ice cubes into it. Observe it for some time. What happens? The ice cubes melt and disappear. Why did it happen?
Solution:
It is because heat energy in the water is transferred to the ice.

Question 2.
Take metal rods of copper, aluminum, brass and iron. Fix a match stick to one end of each rod using a little melted wax. When the temperature of the far ends reaches the melting point of the wax, the matches drop off. It is observed that the match stick on the copper rod would fall first, showing copper as the best conductor followed by aluminum, brass, and then iron.

Aim :
To compare the conducting powers of various metals.

Materials required :
Metal roads of copper, aluminum, brass and iron, match stick, melted wax.

Procedure :
Fix a match stick to one end of each rod using the little melted wax. When the temperature of the far ends reach the melting point of wax, the matches drop. Observe what happens?

Observation :
The match stick on the copper rod would fall first, showing copper as the best conductor followed by aluminum, brass and then iron.

Conclusion:
Metals are good conductors of heat. Copper is the best conductor of heat.

Question 3.
Drop a few crystals of potassium permanganate down to the bottom of a beaker containing water. When the beaker is heated just below the crystals, by a small flame, purple streaks of water rise upwards and fan outwards.
You can do the activity by yourself.

Question 4.
Take some crushed ice cubes in a beaker and note down the temperature using a thermometer. It will be 0°C. Now heat the ice in the beaker. You can observe that ice is melting to form water. Record the temperature at regular intervals and it will remain at 0°C until the whole ice is converted to liquid. Now heat the beaker again and record the temperature. You can notice that the temperature will rise up to 100°C and it will be at 100°C even after continuous heating until the whole mass of water in the beaker is vaporized.
You can do the activity by yourself.

Samacheer Kalvi 9th Science Heat In-Text Problems

Question 1.
Convert the following,

1.  25 °C to Kelvin
2. 200 K to °C

Solution:

1. Tk = T°C + 273.15
Tk = 25 + 273.15 = 298.15 K
2. T°C = Tk – 273.15
T°C = 200 – 273.15 = – 73.15 °C

Question 2.
Convert the following.

1. 35° C to Fahrenheit (°F)
2. 14 °F to °C

Solution:

1. T°F = T°C × 1.8 + 32
T°F = 25° C × 1.8 + 32 = 77 °F
2. T°C = (T°F – 32)/1.8
T°C = (14°F – 32)/1.8 = – 10 °C

Question 3.
Calculate the heat energy required to raise the temperature of 2 kg of water from 10°C to 50°C. The specific heat capacity of water is 4200 JKg– 1 K– 1.
Solution:
Given m = 2 Kg, ∆T = (50 – 10) = 40°C
In terms of Kelvin, ∆T = (323.15 – 283.15) = 40K,
C = 4200 J Kg– 1 K– 1
∴ Heat energy required, Q = m × C × ∆T
= 2 × 4200 × 40
= 3,36,000 J

Question 4.
An iron ball requires 5000 J heat energy to raise its temperature by 20°C. Calculate the heat capacity of the iron ball.
Solution:
Given, Q = 5000 J, ∆T = 20°C or 20 K
Heat Capacity = $$\frac{\text { Heat energy required, } \mathrm{Q}}{\text { Rise in temperature, } \Delta \mathrm{T}}=\frac{5000}{20}$$ = 250 JK– 1

Question 5.
How much heat energy is required to melt 5 kg of ice? (Specific latent heat of ice = 336 Jg– 1)
Solution:
Given, m = 5 Kg = 5000g, L = 336 Jg– 1
Heat energy required = m × L
= 5000 × 336
= 1680000J or 1.68 × 106J

Question 6.
How much boiling water at 100°C is needed to melt 2 kg of ice so that the mixture which is all water is at 0°C?
[Specific heat capacity of water = 4.2 JKg– 1 and specific latent heat of ice = 336 Jg– 1].
Solution:
Given, mass of ice = 2 kg = 2000 g.
Let m be the mass of boiling water required.
Heat lost = Heat gained.
m × c × ∆t = m × L
m × 4.2 × (100 – 0) = 2000 × 336
m = $$\frac{2000 \times 336}{4.2 \times 100}$$
= 1600 g or 1.6 kg.

Samacheer Kalvi 9th Science Heat Additional Questions

Question 1.
Radiation is a method of heat transfer that does not require particles to carry the heat energy.

Question 2.
What is heat energy?
The sum of the kinetic and potential energy is called the internal heat energy of the molecules. This internal energy when flows out is called heat energy.

Question 3.
What are the three scales of temperature?
There are three scales of temperature.

1. Fahrenheit scale
3. Kelvin or Absolute scale.

Question 4.
What is absolute zero?
The temperature at which the pressure and volume of a gas theoretically reach zero is called absolute zero.

Question 5.
What is the concept of temperature?
Temperature is the degree of hotness or coolness of a body. The hotter the body is higher is its temperature.

Question 6.
Differentiate between the three temperature scales.

 Fahrenheit Scale Celcius Scale Kelvin Scale 32°F and 212°F are the freezing and boiling points respectively. 0°C and 100°C are the freezing and boiling points respectively. OK represents absolute zreo. 373.15k and 273.15k are boiling and freezing points respectively. The interval has been divided into 180 parts. The interval has been divided into 100 parts. A one-degree difference in kelvin is equal to a one-degree difference in Celcius. The formula for converting a Fahrenheit scale to a Celcius scale is – C = 5/9(F-32) The formula for converting a Celcius scale to a Fahrenheit scale is – F = 9/5C + 32 The formula for converting a Kelvin scale to a Celcius scale is -C = K-273.15 Also known as the centigrade scale. Also known as an absolute scale.

Question 1.
Write specific heat capacity of any five substances.
Specific heat capacity of a substance is defined as the amount of heat required to raise the temperature of 1 kg of the substance by 1°C or 1 K. The SI unit of specific heat capacity is Jkg– 1K– 1.

Specific Heat Capacity of some common substances

 S. No. Substance Specific Heat Capacity in JKg-1 KT1 1. Lead 130 2. Mercury 139 3. Brass 380 4. Zinc 391 5. Copper 399 6. Iron 483 7. Glass (flint) 504 8. Aluminium 882 9. Kerosene 2100 10. Ice 2100 11. Sea Water 3900 12. Water 4180

Question 2.
Differentiate between Conduction, Convection, and Radiation.

 Conduction Convection Radiation Conduction takes place in solids Convection takes place in liquids and gases. All hot objects give away heat by radiation. Heat transfer takes place on contact between hot to cold molecules. The hot molecules go away from the heat source to the coldest region to the top. Heat is carried as small packets of energy, which travel in straight line. Conduction does not occur in vacuum. Convection does not occur in vacuum. Radiation can occur in vacuum. Heat transfer can occur in any direction from hot to cold body. Heat transfer occurs along the path of convection current from heat source to the coldest region on the top. Heat transfer occurs when photons are met with an obstacle. Conduction is a relatively slow process. This process is faster than conduction but slower than radiation Radiation is the fastest way of heat transfer.

Question 3.
What is the latent heat of vapourisation? Explain with diagram.

Heat energy is absorbed by a solid during melting and an equal amount of heat energy is liberated by the liquid during freezing, without any temperature change. It is called the latent heat of fusion. In the same manner, heat energy is absorbed by a liquid during vaporization and an equal amount of heat energy is liberated by the vapor during condensation, without any temperature changes. This is called the latent heat of vaporization.

Question 4.
Give reasons why –

1. a steam burn is more damaging than a burn caused by boiling water at the same temperature.
2. an igloo is built as a winter shelter
3. gaps are left between railway tracks
4. chimneys are located high up in kitchens and factories
5. we wear woolen clothes in winter.