Nutrition in Animal.

 Nutrition in Animals

Definition: Nutrition is the process by which animals take in and use food to sustain their growth and development.

Types of Nutrition: There are different types of nutrition in animals, including holozoic nutrition, parasitic nutrition, and saprophytic nutrition.

Process of Nutrition

The process of nutrition in animals involves five stages: ingestion, digestion, absorption, assimilation, and egestion.

Ingestion: The intake of food into the body.

Digestion: The breakdown of food into simpler substances.

Absorption: The uptake of soluble substances produced during digestion by the tissues in the body.

Assimilation: The use of simple substances to build complex substances required by the body.

Egestion: The elimination of undigested food from the body.

Nutrition in Amoeba

Amoeba is a single-celled organism that obtains its nutrients by ingesting food particles.

The process of nutrition in Amoeba involves the formation of a food vacuole, digestion, absorption, and egestion.

Human Digestive System

The human digestive system consists of the alimentary canal and other organs such as the gall bladder, pancreas, and liver.

The digestive system breaks down food into simpler substances that can be absorbed and used by the body.

Types of Teeth

There are four different types of teeth:

incisors, canines, premolars, and molars.

Each type of tooth has a specific function, such as biting, tearing, or grinding food.

Digestion in Humans

Digestion starts in the mouth, where food is mixed with saliva that contains digestive enzymes.

The food then passes through the esophagus into the stomach, where it is mixed with digestive juices that break down proteins.

Further digestion takes place in the small intestine, where enzymes from the pancreas and bile from the liver are released.

Absorption and Assimilation

The nutrients absorbed in the blood are transported to the rest of the body.

The final product of carbohydrate digestion, glucose, is broken down into carbon dioxide and water in the cells to release energy.

Amino acids are used for repairing worn-out cells and tissues.

Egestion

The undigested food is eliminated from the body through the anus.

The large intestine absorbs water and minerals, and the remaining waste is stored in the rectum until it is eliminated.

Nutrition in Ruminants

Ruminants are animals that have a four-chambered stomach and digest plant-based foods.

The digestive system of ruminants involves ingestion, digestion, absorption, and egestion.

Ruminants have a unique digestive system that allows them to break down and extract nutrients from plant-based foods.

Nutrition in plants

 Nutrition in Plants

Definition: Nutrition is the process by which plants take in and use food to sustain their growth and development.

Types of Nutrition: There are two main types of nutrition in plants - Autotrophic and Heterotrophic.

Autotrophic Nutrition

Definition: Autotrophic nutrition is the

process by which plants make their own food using sunlight, water, and carbon dioxide.

Process: Photosynthesis is the process by which plants make their own food.

Equation: Carbon dioxide + Water → Glucose + Oxygen (in the presence of sunlight and chlorophyll)

Importance: Autotrophic nutrition is essential for plant growth and development.

Photosynthesis

Definition: Photosynthesis is the process by which plants, algae, and some bacteria convert light energy from the sun into chemical energy in the form of glucose.

Conditions necessary for photosynthesis:

Light

Chlorophyll

Carbon dioxide

Water

Role of chlorophyll: Chlorophyll is a green pigment that plays a crucial role in photosynthesis by absorbing light energy.

Heterotrophic Nutrition

Definition: Heterotrophic nutrition is the process by which plants obtain their nutrients by depending on other organisms.

Types of heterotrophic plants:

Parasitic plants

Saprophytic plants

Insectivorous plants

Symbiotic plants

Parasitic Plants

Definition: Parasitic plants are plants that obtain their nutrients by depending on other plants.

Examples: Cuscuta (dodder), mistletoe

Characteristics: Parasitic plants have special roots that penetrate into the tissues of the host plant.

Saprophytic Plants

Definition: Saprophytic plants are plants that obtain their nutrients from dead and decaying plant and animal matter.

Examples: Indian pipe, coral root

Characteristics: Saprophytic plants have fungi that convert dead and decaying matter into nutrients.

Insectivorous Plants

Definition: Insectivorous plants are plants that obtain their nutrients by trapping and consuming insects.

Examples: Venus flytrap, pitcher plant, sundew

Characteristics: Insectivorous plants have modified leaves that trap and digest insects.

Symbiotic Plants

Definition: Symbiotic plants are plants

that live in association with other organisms and share food and other resources.

Examples: Lichens (symbiotic association between fungi and algae)

Characteristics: Symbiotic plants mutually benefit from each other.

Replenishment of Nutrients in the Soil

Importance: Plants use mineral nutrients from the soil for their growth, leading to depletion of nutrients.

Methods: Manures and fertilizers are used to replenish nutrients in the soil.

Symbiotic association: Rhizobium and leguminous plants have a symbiotic association that replenishes nitrogen in the soil.

Temperature and Heat

 Temperature

Definition: The degree of hotness or coldness of a body or a place is called temperature.

Measurement: Temperature is measured using a thermometer.

Units: Celsius (°C), Fahrenheit (°F), and Kelvin (K) are common units of temperature.

Scales: Celsius scale and Fahrenheit scale are two commonly used temperature scales.

Fixed points: Melting point of ice (0°C or

32°F) and boiling point of water (100°C or 212°F) are used as fixed points to define the temperature scales.

Thermometers

Definition: A thermometer is a device used to measure temperature.

Fact: the first thermometer was invented by galeleo galilei in 1593.

Fact: The human body can perceive temperature difference, but it is not a reliable way to measure temperature accurately. 

Types:

Mercury thermometer: Uses mercury as the thermometric fluid.

Alcohol thermometer: Uses alcohol as the thermometric fluid.

Digital thermometer: Uses a thermistor or other electronic sensor to measure temperature.

Uses: Measuring body temperature, temperature of a substance, and ambient temperature.

Heat

Definition: Heat is a form of energy

that flows from a body at a higher temperature to a body at a lower temperature.

Measurement: Heat energy is measured in calories or joules (J).

Transfer: Heat can be transferred through conduction, convection, and radiation.

Fact:Metal are generally good conductor of heat, while non-metals are poor conductor. 

Modes of Heat Transfer

1. Conduction

Definition: Conduction is the transfer of heat energy through direct contact between particles.

Occurs in: Solids.

Examples: Heat transfer through a metal rod, cooking utensils.

Factors affecting conduction:

Thermal conductivity of the material, temperature difference, and cross-sectional area.

2. Convection

Definition: Convection is the transfer of heat energy through the movement of fluids.

Occurs in: Liquids and gases.

Examples: Sea breeze, land breeze, heating of water in a vessel.

Factors affecting convection: Density difference, temperature difference, and gravity.

Fact: convection current play a crucial role in shaping our climate & weather patterns. 

3. Radiation

Definition: Radiation is the transfer of

heat energy through electromagnetic waves.

Occurs in: Vacuum and medium.

Examples: Heat transfer from the sun, radiation from a fire.

Factors affecting radiation: Temperature, surface area, and emissivity.

Fact: Radiation is the fastest mode of heat transfer and can occur in a vacuum. 

Applications of Heat Transfer

Conduction: Cooking utensils, heat sinks, and thermal insulation.

Convection: Heating of buildings, sea breeze, land breeze, and ocean currents.

Radiation: Solar panels, heating of the Earth's surface, and thermal imaging.

Preventing Heat Loss

Insulation: Using materials that reduce heat transfer.

Thermos flask: A device that minimizes

heat loss through conduction, convection, and radiation.

Vacuum insulation: Using a vacuum to

reduce heat transfer through conduction and convection.

Practical Applications

Solar energy: Harnessing energy from the sun using solar panels.

Thermal insulation: Using materials to

reduce heat transfer in buildings and appliances.

Heat exchangers: Devices that transfer

heat energy from one fluid to another.

Fact;Thermoflascs use vacuum insulation to minimise heat transfer and keep liquids at a consistent temperature. 

Key Concepts

Heat flows from a body at a higher temperature to a body at a lower temperature.

Temperature is a measure of the degree of hotness or coldness of a body.

Different materials have different abilities to conduct heat.

Convection occurs in fluids due to density differences.

Radiation can occur in vacuum and medium.

Acid, base and salt

 Acids

Definition: Substances containing an acid (from Latin "acere" meaning sour)

Types: Mineral acids and organic acids

Mineral Acids

Examples: 

Hydrochloric acid (HCI),

sulphuric acid (H2SO4), and nitric acid (HNO3)

Uses: Laboratory, industrial applications

Properties: Strong, corrosive, and highly reactive towards metals

Organic Acids

Examples: Tartaric acid (grapes), acetic

acid (vinegar), formic acid (sting of ants and bees), malic acid (apples), citric acid (lemons and oranges), lactic acid (milk)

Properties: Weak, naturally occurring in animal and plant materials

Strong and Weak Acids

Strong acids: Highly corrosive, mineral

acids (e.g., hydrochloric acid, sulphuric acid, and nitric acid)

Weak acids: Less destructive, mostly organic acids (e.g., acetic acid)

Properties of Acids

Sour taste

Corrosive nature

Soluble in water

Can be dilute or concentrated

Uses of Acids

Hydrochloric acid (HCI):

Used in industries for heating applications

Cleaning sinks and sanitary ware

Sulphuric acid (H2SO4):

Used in car batteries

Manufacture of paints, drugs, dyes, and fertilizers

Nitric acid (HNO3):

Used by goldsmiths for cleaning gold and silver ornaments

Production of fertilizers

Acetic acid (CH3COOH):

Main ingredient of vinegar

Enhances flavor of food and acts as a preservative in pickles

Used as a cleansing agent

Acidic Environment and Microorganisms

Most microorganisms cannot live in an acidic environment.

Acidic environment can slow down or kill microorganisms.

This is why vinegar is used in many packaged food items like pickles, sauce, and ketchups.

Acid Rain

Acid rain is a major effect of air pollution.

Pollutants like sulphur dioxide and oxides of nitrogen react with atmospheric water and oxygen to form sulphuric acid and nitric acid.

Acid rain can damage plant and animal life, buildings, and monuments.

True or False Statements

1. Acids can be stored in metal containers: False (Acids are corrosive and can react with metals.)

2. Mineral acids are present in animal and plant materials: False (Mineral acids are produced from chemical substances, whereas organic acids are present in animal and plant materials.)

3. A dilute acid has more amount of water than a concentrated acid: True

4. Sulphuric acid is used for cleaning sinks and sanitary ware: False (Hydrochloric acid is used for cleaning sinks and sanitary ware.)

5. Nitric acid is used by goldsmiths for cleaning gold and silver ornaments: True

6. Hydrochloric acid is used to enhance the flavor of food and as a preservative in pickles: False (Acetic acid is used to enhance the flavor of food and as a preservative in pickles.)

Fill in the Blanks

1. Acids are sour to taste.

2. Apples contain malic acid, whereas spinach has oxalic acid.

3. Strong acids are highly corrosive.

4. Organic acids are weak acids.

5. Carbonic acid is present in fizzy drinks and soda water.

Bases

Definition: Substances containing a base are called basic substances.

Examples: Sodium hydroxide (NaOH), calcium hydroxide (Ca(OH)2)

Properties: Bitter taste, slippery feel, may or may not be soluble in water

Strong and Weak Bases

Strong bases: Highly corrosive, can burn skin (e.g., sodium hydroxide, potassium hydroxide)

Weak bases: Less corrosive (e.g., copper hydroxide, zinc hydroxide, ammonium hydroxide)

Uses of Bases

Calcium hydroxide (slaked lime):

Neutralizes acidity in soils

Used in whitewash and mortar

Used in Bordeaux mixture for protecting crops

Magnesium hydroxide (milk of magnesia):

Used as an antacid or laxative

Corrects excess acidity in the stomach

Sodium hydroxide (caustic soda):

Used in manufacture of paper and textiles

Used to unblock drains

Used in manufacture of soaps and detergents

Indicators

Definition: Substances that show a

change in color when brought in contact with acids and bases.

Examples: Litmus, phenolphthalein,

methyl orange

Types: Natural indicators (e.g., turmeric, red cabbage), universal indicators (e.g pH paper)

pH and Universal Indicators

pH: A measure of the strength of an acid or base, ranging from 1 to 14.

Universal indicator: A mixture of indicators that gives a different color for different pH values.

pH paper: A paper soaked in universal indicator solution.

A. Fill in the blanks

1. Strong acids are highly corrosive and can cause severe burns.

2. Bases are slippery to touch.

3. Sulphuric acid is used in the manufacture of paints, dyes, and drugs.

4. Sodium hydroxide is used to unblock drains.

5. Blue litmus changes to red in acids.

B. Choose the correct option

1. d. Sulphuric acid is called the "King of chemicals".

2. c. Acetic acid is present in vinegar.

3. a. Carbonic acid is a weak mineral acid.

4. b. Calamine lotion is used to neutralize bee stings.

5. c. Sugar cannot be used as an indicator.

6. d. Both Potash alum and Silver nitrate are salts.

7. b. Hydrochloric acid is used to remove deposits from the inside of boilers.

8. c. KOH is a strong base.

9. d. pH = 13 represents a strong alkali.

10. a. High melting point is a characteristic property of most salts.

Matching

1. CH3COOH - c. Acetic acid

2. AgNO3 a. Silver nitrate

3. NH4NO3 d. Ammonium nitrate

4. Ca(OH)2 - e. Calcium hydroxide

5. CaCO3 b. Calcium carbonate

Very Short Answer Type Questions

1. Alkalis

2. Indicator

3. pH paper

4. Neutral salt

5. Hydrated salts

Short Answer Type Questions

1. Properties of acids: Sour taste, corrosive nature

Properties of bases:

 Bitter taste, slippery feel

2. Acids or bases are added to soil to adjust its pH for optimal plant growth.

3. Neutralization reaction: A reaction between an acid and a base to form a salt and water. Example: HCI + NaOH NaCl + H2O

4. A hydrated salt can be converted into an anhydrous salt by heating it to remove the water of crystallization. Example: CuSO4.5H20 CuSO4 + 5H2O ←

Long Answer Type Questions

1. Natural indicators can be prepared from plant materials like flowers, roots, stems, and leaves. 

Examples:

Flower: Rose petals

Root: Beetroot

Stem: Turmeric

Leaf: Red cabbage

Red cabbage juice shows different colors in acidic, neutral, and basic mediums: deep red in acidic, purple in neutral, and green/yellow in basic.

2. a. Vinegar is used in packaged food items as a preservative.

b. Slaked lime is added to factory waste to neutralize acidic substances.

c. Magnesium hydroxide is used as an antacid to neutralize excess acid in the stomach.

d. Strong acids and bases should be handled carefully because they can cause severe burns and damage.

3. Water of crystallization: Water molecules present in the crystal structure of a salt. Example: CuSO4-5H2O (copper sulfate pentahydrate

Let's Observe

1. a. Food items: Not specified

b. Process: Not specified

c. Chemical used: Not specified

2. Acidic solution: Turns blue litmus

paper red

Basic solution: Turns red litmus paper blue

Let's Apply

1. Pickles and sauces are not packaged in metal containers because the preservative used (acidic substance) can react with the metal.

2. Hydrochloric acid in the stomach does not corrode the stomach lining because it is highly concentrated and the stomach lining has a protective mechanism.)

Let's Analyse and Evaluate

1. The sanitary ware cleaner likely contained an acidic substance that reacted with the marble flooring, causing discoloration.

2. The cleaner does not spoil sinks and sanitary ware because they are made of materials that can withstand acidic substances, but marble is more sensitive to acidic reactions.

Class 8 chapter 15:Natural phenomena

 Some Natural Phenomena

### Introduction

Natural phenomena are events that occur in nature, often governed by physical laws.

Understanding natural phenomena can help us appreciate the complexity and beauty of the natural world.

### Lightning

1. Formation: Lightning is a massive electrostatic discharge that occurs during thunderstorms.

2. Safety precautions: During lightning storms, it's essential to take safety precautions like avoiding tall objects and staying indoors.

### Earthquakes

1. Causes: Earthquakes are caused by the movement of tectonic plates in the Earth's crust.

2. Effects: Earthquakes can cause destruction, tsunamis, and loss of life.

3. Precautions: During earthquakes, it's essential to take precautions like dropping to the ground and taking cover.

### Conclusion

Natural phenomena like lightning and earthquakes can be fascinating and awe-inspiring, but they also pose significant risks. Understanding these phenomena can help us appreciate the natural world and take necessary precautions.

Chemicals and chemical changes.

Chemical Substances

Types of Chemical Substances

1. Pure Substances: Elements or compounds.

2. Mixtures: Combination of two or more substances not chemically combined.

Elements

1

. Definition: Substance made up of only one kind of atoms.

2.

Properties: Each element has its own distinct set of properties.

3. Examples: Silver, gold, aluminium, hydrogen, oxygen.

Compounds

1. Definition: Substance formed when

two or more elements combine chemically.

2. Properties: Properties of a compound differ from those of its constituent elements.

3. Examples

 Mixtures**

1 . Definition: Combination of two or

more substances not chemically combined.

2

. Properties: Retains properties of its components.

3. Examples: Air, mixture of iron filings and sulphur.

Chemical Symbols

1. Definition: Abbreviations used to represent elements.

2. Purpose: Simplifies writing and communication in chemistry.

Chemical Symbols and Atomicity

History of Chemical Symbols

1. Early Symbols: Pictorial symbols used by John Dalton.

2. Modern System: Developed by Jons Jacob Berzelius using letters of the English alphabet.

Features of Modern Chemical Symbols

1. First Letter: First letter of the element's name is used as its symbol.

2. Additional Letters: Second letter or distinct letter added when necessary.

3. Latin Names: Some symbols derived from Latin names (e.g., Au for Gold, Ag for Silver).

Examples of Chemical Symbols

1. Elements: H (Hydrogen), C (Carbon), O (Oxygen), N (Nitrogen).

2. Symbols from Latin Names: Na (Sodium), K (Potassium), Pb (Lead).

Chemical Formulae and Equations

Chemical Formulae

1. Definition: Representation of a molecule of a compound using chemical symbols of its constituent elements.

2. Examples: H2O (water), NaCl (common salt), CaCO3 (calcium carbonate).

Valency

1. Definition: Combining capacity of an atom of an element.

2. Examples: Hydrogen (1), Oxygen (2), Carbon (4).

Writing Chemical Formulae

1. Steps:

Write symbols of constituent elements.

Write valencies of elements.

Cross over valencies and write as subscripts.

Simplify formula if possible.

Atomicity

1

. Definition: Number of atoms present in one molecule of an element.

2. Types:

Monatomic: 1 atom (e.g., noble gases).

Diatomic: 2 atoms (e.g., oxygen, 02).

Tetratomic: 4 atoms (e.g.,

phosphorus, P4).

Chemical Equations

1 . Definition: Shorthand form of

representing a chemical reaction using symbols and formulae.

2. Components:

Reactants: Substances involved initially in the reaction.

Products: New substances formed in the reaction.

Writing Chemical Equations

1. Steps:

Identify reactants and products.

Write names of reactants on the left-hand side with a '+' sign between them.

Write names of products on the right-hand side with a '+' sign between them.

Use an arrow (→) to separate reactants from products.

Chemical Equations

Writing Chemical Equations

1. Steps:

Identify reactants and products.

Write names of reactants on the left-hand side with a '+' sign between them.

Write names of products on the right-hand side with a '+' sign between them.

Use an arrow (→) to separate reactants from products.

2. Example: Magnesium burns in oxygen to form magnesium oxide.

Word equation: magnesium + oxygen → magnesium oxide

Chemical equation: 2Mg + 02 → 2MgO

Balancing Chemical Equations

1. Definition: Ensuring the number of atoms of each element is equal on both sides of the equation.

2. Steps:

Count the number of atoms of each element on both sides.

Adjust coefficients to balance the equation.

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Chemical equation: 4Fe + 302 + 6H2O → 4Fe(OH)3

Importance of Chemical Equations

1. Representation: Chemical equations

represent chemical reactions in a concise and symbolic way.

2. Balancing: Balancing chemical equations ensures the law of conservation of mass is obeyed

Balancing Chemical Equations

1. Definition: Ensuring the number of atoms of each element is equal on both sides of the equation.

2. Steps:

Count the number of atoms of each element on both sides.

Adjust coefficients to balance the equation.

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Chemical equation: 4Fe + 302 + 6H2O → 4Fe(OH)3

Importance of Chemical Equations

1. Representation: Chemical equations

represent chemical reactions in a concise and symbolic way.

2. Balancing: Balancing chemical equations ensures the law of conservation of mass is obeyed.

Chemical Changes

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Conditions: Oxygen and water are essential for rusting.

Prevention: Oiling or galvanizing iron objects can prevent rusting.

2. Browning of Vegetables and Fruits:

Cut surfaces of vegetables and fruits turn brown due to reaction with atmospheric oxygen.

Prevention: Soaking cut vegetables and fruits in plain water can reduce browning.

3. Reaction between Vinegar and Baking Soda: Produces carbon dioxide gas.

Chemical equation: CH3COOH + NaHCO3 CH3COONa CO2 + H2O +

4. Reaction between Copper Sulphate Solution and Iron Nails: Iron displaces

copper from copper sulphate solution,

forming iron sulphate and copper.

Chemical equation: CuSO4 + Fe → FeSO4 + Cu

Characteristics of Chemical Changes

1. Permanent Change: Chemical

changes are often irreversible.

2. New Substances Formed: Chemical changes result in the formation of new substances with different properties

Physical and Chemical Changes

Physical Changes

1. Definition: Changes in which no new substances are formed.

2. Examples: Formation of ice from water, crystallization of common salt.

3. Characteristics: Properties such as color, shape, size, or physical form may change.

Chemical Changes

1. Definition: Changes in which new substances are formed.

2. Examples: Rusting of iron, reaction

between vinegar and baking soda, reaction between copper sulphate solution and iron nails.

3. Characteristics: Permanent change, new substances formed with different properties.

Crystallization

1. Definition: Process of obtaining crystals of a substance from its solution.

2. Example: Crystallization of common salt from seawater.

3. Steps:

Dissolve impure substance in water.

Filter the solution to remove insoluble impurities.

Allow the solution to cool and form crystals.

Examples of Chemical Reactions

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

2. Reaction between Vinegar and Baking

Soda: Produces carbon dioxide gas.

3. Reaction between Copper Sulphate Solution and Iron Nails: Iron displaces copper from copper sulphate solution, forming iron sulphate and copper.

Understanding secularism

 Secularism: Separation of religion from

the state, ensuring equal treatment of all citizens regardless of their religious beliefs.

Indian Secularism: India adopted a

strategy of separating power from religion and state, preventing any one religion from dominating others.

Objectives:

Prevent one religious community from dominating another.

Ensure the state doesn't enforce any particular religion or take away individual freedom.

Prevent some members from dominating others within the same religious community.

Important Concepts

Secular State: A state that maintains

a principled distance from religion, neither promoting nor interfering with religious practices.

Non-Interference: The state doesn't interfere with religious practices unless they violate fundamental rights or laws.

Intervention: The state may intervene to prevent domination or protect individu rights.

Questions and Answers

1. What is secularism in the Indian context?

Indian secularism refers to the separation of power from religion and state, ensuring equal treatment of all citizens.

2. Why is it important for one religious community not to dominate another?

This ensures equality and prevents tyranny, promoting brotherhood and mutual cooperation.

3. What is the role of the state in promoting secularism? 

The state maintains a principled distance from religion, ensuring equal treatment and preventing domination.

4. Can the government intervene if a religious group says their religion allows infanticide?

Yes, the government can intervene as infanticide is a violation of fundamental rights and laws.

5. What are some examples of secular practices in India?

1.Examples include government schools not promoting any particular religion and laws

2.banning untouchability 

Question 1: Different types of religious practices

People in our neighborhood practice different religions like Hinduism, Islam, Sikhism, and Christianity. They visit temples, mosques, gurudwaras, and churches to pray and worship.

Question 2: Government intervention in infanticide

Yes, the government will stop infanticide because it's a crime and against human rights.

Question 3: Objectives of a secular state

No one religion should dominate another.

The state shouldn't force any particular religion.

Everyone should be equal within their own community.

Question 4: Religious holidays in school calendars

Our school calendar has holidays for different religions like Eid, Diwali, Christmas, and Guru Nanak Jayanti.

Question 5: Different views within the same religion

Yes, there can be different views within the same religion. For example, Hindus worship different gods, and Muslims are divided into Shia and Sunni.

Question 6: Indian state's role in religion

The Indian state respects all religions and doesn't interfere unless someone's rights are violated.

Question 7: Poster on peace and religious tolerance

The poster means that peace requires respecting differences and working together. It promotes harmony and acceptance among people of different religions.