Chemical equations
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The document discusses chemical reactions and how to write chemical equations. It explains that chemical reactions involve rearranging bonds and atoms to form new compounds that are different than the starting materials. It provides examples of word and formula equations and shows the parts of a chemical equation including reactants, products, and physical states. It also instructs how to write chemical equations by converting word equations to symbolic equations using chemical formulas and reaction arrows.
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Chemical equations
The document discusses chemical equations and balancing reactions. It provides examples of chemical equations showing the formation of glucose from carbon dioxide and water during photosynthesis, the formation of carbon dioxide from carbon and oxygen, and the formation of water from hydrogen and oxygen. It also discusses the law of conservation of mass, which states that the total mass of reactants must equal the total mass of products in a chemical reaction.
Writing and balancing chemical reactions
This document discusses writing and balancing chemical reactions. It explains that a chemical equation illustrates the formulas and quantities of reactants and products in a chemical reaction. Guidelines are provided for writing chemical equations, such as writing elements that exist as diatomic molecules and indicating physical states. The document also covers balancing chemical equations using inspection and adjusting coefficients to satisfy the law of conservation of mass. Sample problems demonstrate balancing equations for specific chemical reactions.
Balancing Equations
A chemical equation represents a chemical reaction using formulas to show the reactants and products. It uses coefficients to indicate the ratio in which substances react or are produced, and parentheses to show the state of each substance. A chemical reaction conserves mass according to the law of conservation of mass. There are four main types of chemical reactions: synthesis, decomposition, single replacement, and double replacement.
Notes chemical equations
The document discusses balancing chemical equations by following the law of conservation of mass. It explains that a chemical equation uses symbols to represent a chemical reaction, with reactants on the left side of the yield sign and products on the right. For the equation to be balanced, the number of atoms of each element must be equal on both sides after coefficients are added. This ensures the mass is also conserved, as required by the law of conservation of mass. An example demonstrates balancing the equation for the combustion of propane by adding coefficients to match the number of carbon, hydrogen and oxygen atoms on each side.
Intro to balancing chemical reactions
This document provides instructions for balancing chemical equations. It explains that chemical equations must be balanced to show the same number of atoms of each element on both sides. The steps provided to balance an equation are to: draw boxes around formulas, make an element inventory, and add coefficients to formulas until the inventory is equal on both sides, showing the reaction is balanced. An example reaction and balancing steps are shown. Key aspects are to never change what is in the boxes, keep the inventory updated, and simplify coefficients if possible.
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The document discusses physical and chemical changes, including the key differences between them. A physical change does not create new substances, while a chemical change involves atoms rearranging to form new substances. The document also examines signs that a chemical reaction has occurred, such as a change in color, odor, temperature, or the formation of a gas or precipitate. It introduces the concept of a chemical equation to represent a chemical reaction and explains that chemical equations must be balanced to satisfy the law of conservation of mass.
03 balancing chemical equations
The document discusses the law of conservation of mass and balancing chemical equations. It explains that in a chemical reaction, while the types of atoms may change, the total mass remains the same. It then provides examples of balancing different chemical equations by making the numbers of atoms equal on both sides of the reaction arrow. Methods for balancing include multiplying coefficients and accounting for polyatomic ions.
Chemical reactions and balancing equations
This document discusses chemical reactions and balancing chemical equations. It defines elemental and chemical formulas, and explains that chemical changes occur through breaking and rearrangement of chemical bonds. A chemical equation represents a chemical reaction using formulas to show reactants and products. Parts of a chemical equation include elemental formulas, chemical formulas, coefficients, and subscripts. The document demonstrates how to balance simple chemical equations by making sure the numbers of atoms of each element are equal on both sides of the reaction. It provides steps for balancing equations and examples of balancing practice problems.
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Chemical equations
The document discusses chemical equations and balancing reactions. It provides examples of chemical equations showing the formation of glucose from carbon dioxide and water during photosynthesis, the formation of carbon dioxide from carbon and oxygen, and the formation of water from hydrogen and oxygen. It also discusses the law of conservation of mass, which states that the total mass of reactants must equal the total mass of products in a chemical reaction.
Writing and balancing chemical reactions
This document discusses writing and balancing chemical reactions. It explains that a chemical equation illustrates the formulas and quantities of reactants and products in a chemical reaction. Guidelines are provided for writing chemical equations, such as writing elements that exist as diatomic molecules and indicating physical states. The document also covers balancing chemical equations using inspection and adjusting coefficients to satisfy the law of conservation of mass. Sample problems demonstrate balancing equations for specific chemical reactions.
Balancing Equations
A chemical equation represents a chemical reaction using formulas to show the reactants and products. It uses coefficients to indicate the ratio in which substances react or are produced, and parentheses to show the state of each substance. A chemical reaction conserves mass according to the law of conservation of mass. There are four main types of chemical reactions: synthesis, decomposition, single replacement, and double replacement.
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The document discusses balancing chemical equations by following the law of conservation of mass. It explains that a chemical equation uses symbols to represent a chemical reaction, with reactants on the left side of the yield sign and products on the right. For the equation to be balanced, the number of atoms of each element must be equal on both sides after coefficients are added. This ensures the mass is also conserved, as required by the law of conservation of mass. An example demonstrates balancing the equation for the combustion of propane by adding coefficients to match the number of carbon, hydrogen and oxygen atoms on each side.
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This document provides instructions for balancing chemical equations. It explains that chemical equations must be balanced to show the same number of atoms of each element on both sides. The steps provided to balance an equation are to: draw boxes around formulas, make an element inventory, and add coefficients to formulas until the inventory is equal on both sides, showing the reaction is balanced. An example reaction and balancing steps are shown. Key aspects are to never change what is in the boxes, keep the inventory updated, and simplify coefficients if possible.
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The document discusses physical and chemical changes, including the key differences between them. A physical change does not create new substances, while a chemical change involves atoms rearranging to form new substances. The document also examines signs that a chemical reaction has occurred, such as a change in color, odor, temperature, or the formation of a gas or precipitate. It introduces the concept of a chemical equation to represent a chemical reaction and explains that chemical equations must be balanced to satisfy the law of conservation of mass.
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The document discusses the law of conservation of mass and balancing chemical equations. It explains that in a chemical reaction, while the types of atoms may change, the total mass remains the same. It then provides examples of balancing different chemical equations by making the numbers of atoms equal on both sides of the reaction arrow. Methods for balancing include multiplying coefficients and accounting for polyatomic ions.
Chemical reactions and balancing equations
This document discusses chemical reactions and balancing chemical equations. It defines elemental and chemical formulas, and explains that chemical changes occur through breaking and rearrangement of chemical bonds. A chemical equation represents a chemical reaction using formulas to show reactants and products. Parts of a chemical equation include elemental formulas, chemical formulas, coefficients, and subscripts. The document demonstrates how to balance simple chemical equations by making sure the numbers of atoms of each element are equal on both sides of the reaction. It provides steps for balancing equations and examples of balancing practice problems.
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The document discusses chemical reactions and equations. It provides information on:
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- How chemical equations are used to depict the type and relative amounts of reactants and products in a reaction.
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- The steps to balance chemical equations so that the same number of atoms are on both sides, which is required to satisfy the law of conservation of mass.
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The document discusses different types of chemical reactions including synthesis, decomposition, single displacement, and double displacement reactions. It provides examples of each type of reaction along with balanced chemical equations. It also describes the activity series of metals and how reactivity determines whether single displacement reactions will occur.
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The document discusses how to balance chemical equations by ensuring the total number of atoms on both sides of the equation are equal. It explains that coefficients are used to represent the number of molecules in a reaction, while subscripts indicate the number of atoms in a molecule. The steps to balance an equation are to: 1) Write the unbalanced equation, 2) Count the atoms on each side, 3) Use coefficients to make the atoms equal on both sides. Examples are provided to demonstrate balancing equations through adjusting coefficients and verifying the balanced atoms.
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The document defines key chemical terms like chemical formula, chemical equation, reactants and products. It provides steps for writing a chemical equation, including writing the reaction in words, writing chemical formulae, balancing the equation, and noting states of substances. It gives examples of metals reacting with oxygen to form metal oxides.
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Chemical reactions result in chemical changes where reactants change into new products. Chemical reactions can be written with word equations or symbolic equations. A balanced chemical equation shows that the number of each type of atom is the same on both sides of the reaction, ensuring the law of conservation of mass is followed. Balancing chemical equations involves determining the coefficients needed for the number of atoms to be equal on both sides.
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This document provides key notes on chemical reactions and equations from a 10th grade chemistry textbook. It defines chemical reactions as processes that form new substances with different properties than the reactants. Chemical equations are used to represent chemical reactions symbolically and show the physical states of reactants and products. For equations to be balanced, the number of atoms of each element must be the same on both sides of the reaction. The document also describes several types of chemical reactions including combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. Thermal, electrolytic, and photolytic decomposition reactions are given as examples.
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The document defines key terms related to chemical equations:
- Chemical reactions represent changes where reactants are converted to products through chemical changes.
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- Coefficients indicate the number of atoms or molecular units of each substance involved in the reaction.
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This document defines and describes chemical reactions. It explains that in a chemical reaction, atoms rearrange to form new compounds, with old bonds breaking and new bonds forming. Chemical reactions can be represented by chemical equations that show the reactants and products. Reactions can be exothermic, releasing energy, or endothermic, absorbing energy. They can also vary in reaction rate. The document also covers the law of conservation of matter, balancing chemical equations, and the main types of chemical reactions: synthesis, decomposition, single replacement, double replacement, and combustion reactions.
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This document describes chemical reactions and equations. It discusses:
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The document discusses chemical reactions and equations. It defines chemical reactions as chemical changes where bonds in reactants break and products form. It also lists several types of chemical reactions including synthesis, decomposition, single replacement, and combustion. The document emphasizes the importance of balancing chemical equations so that mass is conserved in reactions according to the law of conservation of mass.
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Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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Chemical equations
- 1. Section 2.6—Chemical Reactions If we’re going to do chemical reactions with antacids, we’d better know how to write them!
- 2. Chemical Reactions Watch as 2 H 2 and 1 O 2 undergo a chemical reaction Bonds and atoms are rearranged to form new compounds. 2 H 2 + O 2 2 H 2 O O O H H H H
- 3. Chemical Reactions Bonds and atoms are rearranged to form new compounds. The compounds in the end are different from those in the beginning Bonds are broken and formed between different atoms 2 H 2 + O 2 2 H 2 O O O H H O H H O H H H H
- 4. Chemical Equations The “sentence” of chemistry that shows how the starting materials and the final products of a chemical reaction
- 5. Examples of Chemical Equations Word equation: magnesium metal is reacted with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas Visualization Formula equation: Mg (s) + 2 HCl (aq) MgCl 2 (aq) + H 2 (g)
- 6. Parts of a Chemical Equation NaCl (aq) + AgNO 3 (aq) AgCl(s) + NaNO 3 (aq) Reactants States of matter Arrow Products The starting materials for the reaction—each compound is separated by a “+” s = solid l = liquid g = gas aq = aqueous (dissolved in water) Read as: Yields Produces Forms Makes etc. Formed in the reaction
- 8. Let’s Practice #1 Example: Write the word equation into symbol form Aluminum metal is reacted with hydrochloric acid to form aluminum chloride and hydrogen gas
- 9. Let’s Practice #1 Aluminum metal is reacted with hydrochloric acid to form aluminum chloride and hydrogen gas Al + HCl AlCl 3 + H 2 Example: Write the word equation into symbol form
- 10. Let’s Practice #2 Example: Write the word equation into symbol form Copper (II) nitrate and sodium hydroxide form copper (II) hydroxide and sodium nitrate
- 11. Let’s Practice #2 Copper (II) nitrate and sodium hydroxide form copper (II) hydroxide and sodium nitrate Cu(NO 3 ) 2 + NaOH Cu(OH) 2 + NaNO 3 Example: Write the word equation into symbol form